The Structure of an Atom

Size: px
Start display at page:

Download "The Structure of an Atom"

Transcription

1 CP Biology 2016 Name KEY UNIT 2A: Basic Chemistry Chapter 2: The Chemistry of Life 2.1 The Nature of Matter The Structure of an Atom Living things share a major fundamental similarity with nonliving matter. All matter is made up of atoms. *Atom: the basic unit of all matter Atoms are incredibly small in size, yet they themselves are made of even smaller subatomic particles called protons, neutrons and electrons. Protons and Neutrons have about the same mass but not the same electrical charge. Protons and neutrons are bound by strong forces which form the nucleus or center of the atom. The electron is a charged particle with 1/1840 th the mass of a proton. The energy of their constant motion keeps them outside the nucleus, despite their attraction to the nucleus. Because atoms have equal numbers of electrons and protons, their positive and negative charges balance out and atoms themselves are electrically neutral. Complete the Chart Below: Subatomic Electrical Location Particle Charge within atom proton +1 positive nucleus neutron 0 neutral electron -1 negative nucleus Moving rapidly in energy levels (electron cloud) surrounding the nucleus Your personal notes, summary of the lesson, and/or questions that you may have: 1

2 A chemical Element is a pure substance that consists entirely of one type of atom. More than 100 elements are known, but only about two dozen are commonly found in living organisms. The Periodic Table of Elements (see picture of periodic table on the last page) The Periodic Table of Elements is a reference tool we use to gain information about different elements. Elements are arranged in order by their atomic number. By using the periodic table we can determine 3 things: 1) Element Name and Symbol a symbol is usually 1 or 2 letter abbreviation for the element s name. 2) Mass Number this is the sum of the protons and the neutrons in the nucleus. The electrons don t count in the mass since their mass is next to nothing. 3) Atomic Number the number of protons in the nucleus of an element. Important Biological Elements The five most abundant elements in living things are: 1. Hydrogen 10% 2. Oxygen 65% 3. Nitrogen 4% 4. Carbon 19% 5. Phosphorus 1% Your personal notes, summary of the lesson, and/or questions that you may have: Element Name and Symbol 1) C is the symbol for Carbon 2) Na is the symbol for Sodium Mass Number You may see a decimal number for the mass on the periodic table because this is the average mass for the atoms of this element. Some atoms differ slightly in mass due to different number of neutrons. These are called isotopes and will be studied next year in Chemistry. For Biology class we will round this number to the nearest whole number. 3) The mass of Oxygen is 16 amu 4) The mass of Chlorine is 35 amu Atomic Number 5) The atomic number of Hydrogen is 1 6) The atomic number of Sodium is 11 Protons and Electrons 7) Carbon has 6 protons and 6 electrons. 8) Lithium has 3 protons and 3 electrons. Label the Important Biological Elements 2

3 Chemical Compounds In nature, it is common to find elements combined with other elements in compounds. *Compounds / molecules: a substance formed by the chemical combination of two or more elements in definite proportions. *Coefficient: tells how many molecules of that substance (the large number BEFORE the formula) *Subscript: goes with the element symbol preceding the number; tells how many atoms of that element within one molecule of the substance (small number WITHIN the formula. The physical and chemical properties of a compound are usually very different from those of the original elements from which it is formed. Example : NaCl (Table Salt) NaCl is formed from one atom of sodium a highly reactive, soft, silver-colored metal AND one atom of chlorine a poisonous yellow-green gas. Chemical formulas tell us: a) They types of elements (atoms) that are present in the compound. b) The number of atoms of each element present in the compound. Your personal notes, summary of the lesson, and/or questions that you may have: We show the composition of chemical compounds by a kind of shorthand known as a chemical formula. Example 1: What is the chemical formula for water which contains two hydrogen atoms and one oxygen atom? H 2 O Example 2: 6CO 2 a) What is the coefficient? 6 b) What is carbon s subscript? 1 c) What is oxygen s subscript? 2 d) How many molecules of this compound are represented by this formula? 6 e) How many atoms TOTAL are present in this molecule? 18 Use the following information on chemical names and chemical formulas to fill in the chart below: Carbon 1 Hydrogen - 4 Hydrogen 2 Oxygen - 1 Carbon - 1 Oxygen - 2 Nitrogen - 1 Hydrogen - 3 3

4 Chemical Bonds The atoms in compounds are held together by various types of chemical bonds. Bond formation involves the electrons that surround each atomic nucleus. *Valence Electrons: the electrons in an atom that are available to form bonds (these are unpaired electrons which are found in the outermost energy level of the atom s electron cloud). *Octet Rule: the outermost energy level of most atoms will be complete when containing 8 electrons. Atoms will tend to gain, lose, or share electrons to achieve stability by having a full outer energy level (stable octet). Exception: for hydrogen, the Duet rule applies (only 2 electrons are needed in the valence level) ~ Do you think Carbon, Oxygen, Nitrogen and Hydrogen are reactive (unstable) atoms? Explain. Yes, in each case, there is a vacancy in the outer energy level. H has one vacancy in the 1 st energy level. O has 2 vacancies in the 2 nd energy level. Nitrogen has 3 vacancies and Carbon has 4. ~ What can reactive /unstable atoms do to become nonreactive /stable? (Recall that a stable atom has a fully filled outer energy level.) They can interact with other atoms by gaining, losing or sharing electrons to complete the atom s valence energy level. The main type of bond that we will study in the unit is the covalent bond. Only reactive atoms are able to form bonds. The reactivity of an atom depends upon the arrangement of electrons in its outmost (or valence) energy level. Your personal notes, summary of the lesson, and/or questions that you may have: 4

5 *Covalent Bonds Formed when nonmetal atoms bond with each other A bond in which moving electrons actually travel about the nuclei of two atoms (at the same time) Electrons are shared between two atoms Example 1: Water (H 2 O) Single Covalent Bond: atoms share 2 electrons (1 pair) Double Covalent Bond: atoms share 4 electrons (2 pairs) Triple Covalent Bond: atoms share 6 electrons (3 pairs) *Molecule: the structure that results when atoms are joined together by covalent bonds. The smallest unit of most compounds. NOTE: Bonds between the biologically important atoms H, O, N, C, & P (all non-metals) will be covalent. Hydrogen will only form Covalent Bonds!! H O N C Molecules can also be represented by Structural Formulas: a drawing that shows the arrangement of atoms in a molecule Example 2: Methane (CH 4 ) Structural Formulas tell you: a) the types of elements in the molecule b) the number of atoms of each element AND c) the arrangement of atoms and location of covalent bonds. Shows the two dimensional shape of the molecule. Your personal notes, summary of the lesson, and/or questions that you may have: 5

6 NOTE: Structural formulas usually represent covalent bonding so they are used for molecules like H 2 O, but not for formula units like NaCl. In a structural formula, each line between atoms represent a position in which electrons are shared. Therefore, a line represents a single covalent bond. 1) Hydrochloric Acid (Hydrogen Chloride) or HCl 1 atoms of Hydrogen in the molecule 1 atoms of Chlorine in the molecule 2) Ammonia or NH 3 1 atoms of Nitrogen in the molecule 3 atoms of Hydrogen in the molecule H N H H - Cl H 3) Oxygen gas or O 2 2 atoms of Oxygen in the molecule 4) Carbon Dioxide or CO 2 1 atoms of Carbon in the molecule 2 atoms of Oxygen in the molecule O = O O = C = O Your personal notes, summary of the lesson, and/or questions that you may have: 6

7 2.4 Chemical Reactions Note: We will not be discussing Enzymes in this unit. *Chemical Reactions: process that changes or transforms one set of chemicals into another set of chemicals. Involves changes to the chemical bonds that join atoms in compounds. The numbers and types The numbers and types of atoms in the = of atoms in the reactants products Bonds of the reactants are broken and new bonds form in the products. *Reactants: elements or compounds that enter into a chemical reaction *Products: elements or compounds produced by a chemical reaction HINT: Reactants react to produce products! Use the chemical formulas below to determine how many atoms of each element make up each compound. A coefficient indicates the number of molecules present. (coefficient X subscript = the number of atoms) *Chemical Equations: a mathematical representation of a chemical reaction. It shows the numbers and types of compounds involved. *The Law of Conservation of Matter: matter (atoms and elements) in a chemical reaction cannot be created nor destroyed. Only the arrangement of the atoms is changed, NOT the number or types. Your personal notes, summary of the lesson, and/or questions that you may have: 7

8 Consider the following chemical equation for cellular respiration: In the diagram below, fill in the terms products or reactants in the proper blanks. 6O 2 + C 6 H 12 O 6 6CO 2 + 6H 2 O Reactants C 6, H 12, O 18 Products C 6, H 12, O 18 Your personal notes, summary of the lesson, and/or questions that you may have: 8

9 CP Biology Name PRACTICE PACKET General Chemistry

10 #1 Periodic Table Use the following terms to fill in the blanks for questions 1-8: protons mass number neutrons energy levels nucleus symbol electrons atomic number 1) The periodic table is arranged in general order of increasing a), b) and, c). 2) Each element in the table has a different a), b), c), and d). 3) The number of protons in the nucleus of an atom is the same as the a), and b). 4) The large letter(s) that represent each element is called a. Complete the diagram by labeling all the parts. 5) 6) Made up of 7) and 8) 9) 12) Complete the following table by placing a check in each box that makes the statement true: Characteristic Electron Proton Neutron Has nearly no mass Positively charged Found in the nucleus Moves in energy levels Added together to make the mass number or atomic mass (weight) Does not have an electrical charge Negatively charged

11 13) Use the Periodic Table of the Elements to complete the following table. Note: Add the names and information for three elements of your own choosing: ELEMENT SYMBOL ATOMIC NUMBER MASS NUMBER * NUMBER OF PROTONS NUMBER OF ELECTRONS HYDROGEN H 1 NITROGEN CARBON 12 Na CHLORINE Cl 17 SILVER Pick 3 more elements: *Note: Remember to round off the atomic weight to obtain the mass number or atomic mass. In any neutral atom, the number of is always equal to the number of.

12 #2 Subatomic Particles You will become more familiar with the atomic structure of some atoms by completing the chart below. For each element, you have been given enough information to fill in all the blanks. Use the periodic Table. Element Symbol Atomic Number Mass Number Number of Protons Numbers of Neutrons Number of Electrons Helium He Iodine I Neon Ne Zirconium Zr Aluminum Al Zn Kr Calcium 40 B 5 Sodium ion Na S 2- Chlorine Ion Hydrogen Ion 1 0 (no, it s not a typo)

13 #3 Reactivity of Atoms In biology we are concerned about how atoms join each other to form molecules like hydrogen gas (H 2 ), carbon dioxide (CO 2 ) and glucose (C 6 H 12 O 6 ). The tendency of atoms to bond with each other depends on their reactivity. The reactivity or combining capacity of an atom depends upon the arrangement of electrons in the outermost energy level, known as the valence. Circle the correct term in parenthesis for each sentence below. 1. If an atom s outermost energy level is completely filled with electrons (no vacancies), the atom considered ( stable / unstable ) and nonreactive. Therefore, it ( will / will not ) form bonds with other atoms. List three examples of nonreactive elements: On the Periodic Table, where do we find the nonreactive elements? Nonreactive elements are also known as the Gases. 2. If an atom s outermost energy level is not completely filled with electrons (vacancies present), the atom is considered ( stable / unstable ) and reactive. Therefore, it ( will / will not ) combine with other atoms. Examples of reactive atoms: Element Symbol Atomic Number # electrons Draw the electrons in their energy levels Reactive (R) or non-reactive (NR) Carbon C Hydrogen H Oxygen O Nitrogen N Magnesium Mg Silicon Si Chlorine Cl Argon Ar

14 #4 Electrons and the Reactivity of Atoms Directions: Place the answer to the following questions on the line provided. 1. Energy levels are: a. the charge of protons c. the definite locations of electrons b. the charge of atoms d. the probable locations of electrons 2. If an atom is reactive, how does it become stable? a. join a water molecule b. join the nuclei of other atoms c. form energy levels with other subatomic particles d. form bonds with other reactive atoms Directions: Smiley Cyrus was a student at Livingston High School. Below are her drawings of Bohr models for atoms of three different elements. Check Smiley Cyrus s work each diagram has TWO mistakes. Your task is to fix her errors. * P=protons N=neutrons E= Electrons = electrons in energy levels Nitrogen Argon Hydrogen Circle the atom(s) below that are reactive. Put a triangle around the atom(s) below that are nonreactive. N Ar H K C O He How many electron vacancies are in the valence of each of the following atoms? N Ar H K C O He

15 #5 Bohr Models and Lewis Dot Structures 1. What is the maximum number of electrons that can be found in the first energy level? 2. What is the maximum number of electrons that can be found in the second energy level? 3. For any atom with an atomic number greater than 2, the maximum number of electrons that can be found in the outermost energy level (valence) is:. This is known as the Octet Rule. An atom with a full valence is nonreactive and stable. 4. Draw a Bohr Model and Lewis Dot Structure for each element below. Follow the example given. Element Bohr Model Lewis Dot Structure Number of electron vacancies in valence Sulfur (S) 2 Phosphorous(P) Fluorine (F) Neon (Ne) Lithium (Li)

16 #6 Bonding Patterns 1) What is the purpose of bonding? 2) Is one atom of carbon stable? Why or why not? 3) How many electrons will an atom of carbon share with another atom in order to become stable? 4) List the two most common types of bonds that can form between atoms: a) (sharing of e-) b) (transfer of e-) 5) A is a shorthand way of showing the types and numbers of atoms in a molecule or compound. For example, H 2 O indicates that one atom of oxygen has bonded with two atoms of hydrogen. Circle the correct term in parenthesis: The ( coefficient, subscript ) indicates how many atoms of the preceding element are found in the molecule. The (coefficient, subscript ) indicates how many molecules of each compound are present. In order to determine the number of atoms in a formula with a coefficient, ( multiply, add, divide ) the coefficient and the subscript. Any time you don t see a coefficient, you can assume it is 1 ; the same is true for a subscript. (example: the chemical formula CO 2 indicates one molecule of carbon dioxide which contains one atom of carbon and two atoms of oxygen). Complete in the following chart: Chemical Formula 2H 2 O CaCO 3 2H 2 O 6H 2 SO 4 Total Number of atoms of each element Four hydrogen atoms and two oxygen atoms. Directions for drawing structural formulas: A structural formula is a drawing of the atoms in a compound and the number of bonds between atoms. The short lines in a structural formula represent a covalent bond (or a shared pair of e-) that has formed between two atoms. A single bond is represented by a single line (-). A double bond is shown with two lines (=). A triple bond would contain 3 lines ( ). Example H 2 O or water : One water molecule contains atom(s) of hydrogen and atom(s) of oxygen. Hydrogen (H) has one electron and one vacancy in its valence. So, it needs bond(s) to be stable. Oxygen (O) has six electrons in its valence (which means 2 vacancies). So, it needs bond(s) to be stable. By joining together, the atoms can share electrons in a way that makes all three atoms stable, each with a full valence. The compound is stable and neutral overall because the total #p is still equal to the total #e-. The way to represent this is to draw: H O H In this way, the two atoms of hydrogen are bonded with one atom of oxygen. The hydrogen atoms each have one bond and the oxygen atom has two bonds.

17 Try these examples: Draw the structural formulas for the following compound. Follow the models. H 2 # bonds each hydrogen can form? 1 N 2 # bonds each nitrogen can form? H H CH 4 # bonds carbon can form? each hydrogen? H 2 O 2 # bonds each hydrogen can form? each oxygen? PCl 3 # bonds needed by each phosphorus? each Cl? O 2 # bonds needed by each oxygen? HCN (Hydrogen cyanide) H 2 O

18 #7 Counting Atoms Calculate how many atoms of each element are present in each of the following (as written). 1. 3NaHCO C 2 H 4 O Mg(OH) H 3 PO 4 5. H 2 SO 4 6. (NH 4 ) 3 PO 4 7. C 6 H 12 O CaCO 3

19 #8 Recognizing Balanced Equations Remember, in a balanced chemical equation, the number of atoms of each element in the reactants will equal the number of atoms of each element in the products. EQUATION IS IT BALANCED, as written? (Y/N) A. 2C 2 H 6 + 5O 2 --> 2CO 2 + 6H 2 O B. 2H 2 O 2 --> 2H 2 O + O 2 C. Na + O 2 --> 2Na 2 O D. N 2 + 3H 2 --> 2NH 3 E. P 4 + 5O 2 --> P 4 O 10 F. 3Fe + 4H 2 O --> Fe 3 O 4 + 4H 2 G. C + 2H 2 --> CH 4 H. Al 2 O 3 --> Al + 3O 2 I. H 2 + O 2 --> H 2 O 2 J. Na 2 SO 4 + CaCl 2 --> CaSO 4 + 2NaCl

20 #9 Balancing Equations Answer the following questions. Use complete sentences when given one or more lines to respond. State the Law of Conservation of Matter: To balance an equation, coefficient(s) may be added/removed/changed but subscripts cannot. Balance each of the following equations. H 2 + Cl 2 HCl Fe + O 2 Fe 2 O 3 C 6 H 12 O 6 + O 2 CO 2 + H 2 O H 2 O + Cl 2 O 3 HClO 2 C 6 H 6 + O 2 CO 2 + H 2 O 1) What is meant by the terms: products and reactants in a chemical equation? How do we know which is which? 2) Explain what the subscript indicates. What does it mean if there is no subscript? 3) Explain what the coefficient indicates. What does it mean if there is no coefficient? 4) Explain why chemical equations must be balanced.

Test Bank - Chapter 4 Multiple Choice

Test Bank - Chapter 4 Multiple Choice Test Bank - Chapter 4 The questions in the test bank cover the concepts from the lessons in Chapter 4. Select questions from any of the categories that match the content you covered with students. The

More information

Chapter 2 The Chemical Context of Life

Chapter 2 The Chemical Context of Life Chapter 2 The Chemical Context of Life Multiple-Choice Questions 1) About 25 of the 92 natural elements are known to be essential to life. Which four of these 25 elements make up approximately 96% of living

More information

7.4. Using the Bohr Theory KNOW? Using the Bohr Theory to Describe Atoms and Ions

7.4. Using the Bohr Theory KNOW? Using the Bohr Theory to Describe Atoms and Ions 7.4 Using the Bohr Theory LEARNING TIP Models such as Figures 1 to 4, on pages 218 and 219, help you visualize scientific explanations. As you examine Figures 1 to 4, look back and forth between the diagrams

More information

Untitled Document. 1. Which of the following best describes an atom? 4. Which statement best describes the density of an atom s nucleus?

Untitled Document. 1. Which of the following best describes an atom? 4. Which statement best describes the density of an atom s nucleus? Name: Date: 1. Which of the following best describes an atom? A. protons and electrons grouped together in a random pattern B. protons and electrons grouped together in an alternating pattern C. a core

More information

PROTONS AND ELECTRONS

PROTONS AND ELECTRONS reflect Imagine that you have a bowl of oranges, bananas, pineapples, berries, pears, and watermelon. How do you identify each piece of fruit? Most likely, you are familiar with the characteristics of

More information

List the 3 main types of subatomic particles and indicate the mass and electrical charge of each.

List the 3 main types of subatomic particles and indicate the mass and electrical charge of each. Basic Chemistry Why do we study chemistry in a biology course? All living organisms are composed of chemicals. To understand life, we must understand the structure, function, and properties of the chemicals

More information

Chapter 2: The Chemical Context of Life

Chapter 2: The Chemical Context of Life Chapter 2: The Chemical Context of Life Name Period This chapter covers the basics that you may have learned in your chemistry class. Whether your teacher goes over this chapter, or assigns it for you

More information

Name: Teacher: Pd. Date:

Name: Teacher: Pd. Date: Name: Teacher: Pd. Date: STAAR Tutorial : Energy and Matter: Elements, Compounds, and Chemical Equations: 6.5C Differentiate between elements and compounds on the most basic level. 8.5F Recognize whether

More information

20.2 Chemical Equations

20.2 Chemical Equations All of the chemical changes you observed in the last Investigation were the result of chemical reactions. A chemical reaction involves a rearrangement of atoms in one or more reactants to form one or more

More information

Chapter 5 TEST: The Periodic Table name

Chapter 5 TEST: The Periodic Table name Chapter 5 TEST: The Periodic Table name HPS # date: Multiple Choice Identify the choice that best completes the statement or answers the question. 1. The order of elements in the periodic table is based

More information

19.1 Bonding and Molecules

19.1 Bonding and Molecules Most of the matter around you and inside of you is in the form of compounds. For example, your body is about 80 percent water. You learned in the last unit that water, H 2 O, is made up of hydrogen and

More information

Molecular Models in Biology

Molecular Models in Biology Molecular Models in Biology Objectives: After this lab a student will be able to: 1) Understand the properties of atoms that give rise to bonds. 2) Understand how and why atoms form ions. 3) Model covalent,

More information

2 The Structure of Atoms

2 The Structure of Atoms CHAPTER 4 2 The Structure of Atoms SECTION Atoms KEY IDEAS As you read this section, keep these questions in mind: What do atoms of the same element have in common? What are isotopes? How is an element

More information

UNIT (2) ATOMS AND ELEMENTS

UNIT (2) ATOMS AND ELEMENTS UNIT (2) ATOMS AND ELEMENTS 2.1 Elements An element is a fundamental substance that cannot be broken down by chemical means into simpler substances. Each element is represented by an abbreviation called

More information

Unit 3 Study Guide: Electron Configuration & The Periodic Table

Unit 3 Study Guide: Electron Configuration & The Periodic Table Name: Teacher s Name: Class: Block: Date: Unit 3 Study Guide: Electron Configuration & The Periodic Table 1. For each of the following elements, state whether the element is radioactive, synthetic or both.

More information

Bonding Practice Problems

Bonding Practice Problems NAME 1. When compared to H 2 S, H 2 O has a higher 8. Given the Lewis electron-dot diagram: boiling point because H 2 O contains stronger metallic bonds covalent bonds ionic bonds hydrogen bonds 2. Which

More information

neutrons are present?

neutrons are present? AP Chem Summer Assignment Worksheet #1 Atomic Structure 1. a) For the ion 39 K +, state how many electrons, how many protons, and how many 19 neutrons are present? b) Which of these particles has the smallest

More information

Atoms and Molecules. Preparation. Objectives. Standards. Materials. Grade Level: 5-8 Group Size: 20-30 Time: 60 90 Minutes Presenters: 2-4

Atoms and Molecules. Preparation. Objectives. Standards. Materials. Grade Level: 5-8 Group Size: 20-30 Time: 60 90 Minutes Presenters: 2-4 Atoms and Molecules Preparation Grade Level: 5-8 Group Size: 20-30 Time: 60 90 Minutes Presenters: 2-4 Objectives This lesson will enable students to: Describe how atoms are the building blocks of matter

More information

47374_04_p25-32.qxd 2/9/07 7:50 AM Page 25. 4 Atoms and Elements

47374_04_p25-32.qxd 2/9/07 7:50 AM Page 25. 4 Atoms and Elements 47374_04_p25-32.qxd 2/9/07 7:50 AM Page 25 4 Atoms and Elements 4.1 a. Cu b. Si c. K d. N e. Fe f. Ba g. Pb h. Sr 4.2 a. O b. Li c. S d. Al e. H f. Ne g. Sn h. Au 4.3 a. carbon b. chlorine c. iodine d.

More information

Sample Exercise 8.1 Magnitudes of Lattice Energies

Sample Exercise 8.1 Magnitudes of Lattice Energies Sample Exercise 8.1 Magnitudes of Lattice Energies Without consulting Table 8.2, arrange the ionic compounds NaF, CsI, and CaO in order of increasing lattice energy. Analyze From the formulas for three

More information

Ionic and Metallic Bonding

Ionic and Metallic Bonding Ionic and Metallic Bonding BNDING AND INTERACTINS 71 Ions For students using the Foundation edition, assign problems 1, 3 5, 7 12, 14, 15, 18 20 Essential Understanding Ions form when atoms gain or lose

More information

Sample Exercise 8.1 Magnitudes of Lattice Energies

Sample Exercise 8.1 Magnitudes of Lattice Energies Sample Exercise 8.1 Magnitudes of Lattice Energies Without consulting Table 8.2, arrange the following ionic compounds in order of increasing lattice energy: NaF, CsI, and CaO. Analyze: From the formulas

More information

******* KEY ******* Atomic Structure & Periodic Table Test Study Guide

******* KEY ******* Atomic Structure & Periodic Table Test Study Guide Atomic Structure & Periodic Table Test Study Guide VOCABULARY: Write a brief definition of each term in the space provided. 1. Atoms: smallest unit of an element that has all of the properties of that

More information

Periodic Table Questions

Periodic Table Questions Periodic Table Questions 1. The elements characterized as nonmetals are located in the periodic table at the (1) far left; (2) bottom; (3) center; (4) top right. 2. An element that is a liquid at STP is

More information

7-5.5. Translate chemical symbols and the chemical formulas of common substances to show the component parts of the substances including:

7-5.5. Translate chemical symbols and the chemical formulas of common substances to show the component parts of the substances including: 7-5.5 Translate chemical symbols and the chemical formulas of common substances to show the component parts of the substances including: NaCl [salt], H 2 O [water], C 6 H 12 O 6 [simple sugar], O 2 [oxygen

More information

B) atomic number C) both the solid and the liquid phase D) Au C) Sn, Si, C A) metal C) O, S, Se C) In D) tin D) methane D) bismuth B) Group 2 metal

B) atomic number C) both the solid and the liquid phase D) Au C) Sn, Si, C A) metal C) O, S, Se C) In D) tin D) methane D) bismuth B) Group 2 metal 1. The elements on the Periodic Table are arranged in order of increasing A) atomic mass B) atomic number C) molar mass D) oxidation number 2. Which list of elements consists of a metal, a metalloid, and

More information

ATOMS A T O M S, I S O T O P E S, A N D I O N S. The Academic Support Center @ Daytona State College (Science 120, Page 1 of 39)

ATOMS A T O M S, I S O T O P E S, A N D I O N S. The Academic Support Center @ Daytona State College (Science 120, Page 1 of 39) ATOMS A T O M S, I S O T O P E S, A N D I O N S The Academic Support Center @ Daytona State College (Science 120, Page 1 of 39) THE ATOM All elements listed on the periodic table are made up of atoms.

More information

Chemical Calculations: Formula Masses, Moles, and Chemical Equations

Chemical Calculations: Formula Masses, Moles, and Chemical Equations Chemical Calculations: Formula Masses, Moles, and Chemical Equations Atomic Mass & Formula Mass Recall from Chapter Three that the average mass of an atom of a given element can be found on the periodic

More information

Balancing Chemical Equations

Balancing Chemical Equations Balancing Chemical Equations Academic Success Center Science Tutoring Area Science Tutoring Area Law of Conservation of Mass Matter cannot be created nor destroyed Therefore the number of each type of

More information

ANSWER KEY : BUILD AN ATOM PART I: ATOM SCREEN Build an Atom simulation ( http://phet.colorado.edu/en/simulation/build an atom )

ANSWER KEY : BUILD AN ATOM PART I: ATOM SCREEN Build an Atom simulation ( http://phet.colorado.edu/en/simulation/build an atom ) ANSWER KEY : PART I: ATOM SCREEN Build an Atom simulation ( http://phet.colorado.edu/en/simulation/build an atom ) 1. Explore the Build an Atom simulation with your group. As you explore, talk about what

More information

Lewis Dot Structures of Atoms and Ions

Lewis Dot Structures of Atoms and Ions Why? The chemical properties of an element are based on the number of electrons in the outer shell of its atoms. We use Lewis dot structures to map these valence electrons in order to identify stable electron

More information

Chapter 2 Atoms, Ions, and the Periodic Table

Chapter 2 Atoms, Ions, and the Periodic Table Chapter 2 Atoms, Ions, and the Periodic Table 2.1 (a) neutron; (b) law of conservation of mass; (c) proton; (d) main-group element; (e) relative atomic mass; (f) mass number; (g) isotope; (h) cation; (i)

More information

Topic 4 National Chemistry Summary Notes. Formulae, Equations, Balancing Equations and The Mole

Topic 4 National Chemistry Summary Notes. Formulae, Equations, Balancing Equations and The Mole Topic 4 National Chemistry Summary Notes Formulae, Equations, Balancing Equations and The Mole LI 1 The chemical formula of a covalent molecular compound tells us the number of atoms of each element present

More information

Lewis Dot Notation Ionic Bonds Covalent Bonds Polar Covalent Bonds Lewis Dot Notation Revisited Resonance

Lewis Dot Notation Ionic Bonds Covalent Bonds Polar Covalent Bonds Lewis Dot Notation Revisited Resonance Lewis Dot Notation Ionic Bonds Covalent Bonds Polar Covalent Bonds Lewis Dot Notation Revisited Resonance Lewis Dot notation is a way of describing the outer shell (also called the valence shell) of an

More information

Name Block Date Ch 17 Atomic Nature of Matter Notes Mrs. Peck. atoms- the smallest particle of an element that can be identified with that element

Name Block Date Ch 17 Atomic Nature of Matter Notes Mrs. Peck. atoms- the smallest particle of an element that can be identified with that element Name Block Date Ch 17 Atomic Nature of Matter Notes Mrs. Peck atoms- the smallest particle of an element that can be identified with that element are the building blocks of matter consists of protons and

More information

Ionic and Covalent Bonds

Ionic and Covalent Bonds Ionic and Covalent Bonds Ionic Bonds Transfer of Electrons When metals bond with nonmetals, electrons are from the metal to the nonmetal The becomes a cation and the becomes an anion. The between the cation

More information

Trends of the Periodic Table Basics

Trends of the Periodic Table Basics Trends of the Periodic Table Basics Trends are patterns of behaviors that atoms on the periodic table of elements follow. Trends hold true most of the time, but there are exceptions, or blips, where the

More information

Elements in the periodic table are indicated by SYMBOLS. To the left of the symbol we find the atomic mass (A) at the upper corner, and the atomic num

Elements in the periodic table are indicated by SYMBOLS. To the left of the symbol we find the atomic mass (A) at the upper corner, and the atomic num . ATOMIC STRUCTURE FUNDAMENTALS LEARNING OBJECTIVES To review the basics concepts of atomic structure that have direct relevance to the fundamental concepts of organic chemistry. This material is essential

More information

Trends of the Periodic Table Diary

Trends of the Periodic Table Diary Trends of the Periodic Table Diary Trends are patterns of behaviors that atoms on the periodic table of elements follow. Trends hold true most of the time, but there are exceptions, or blips, where the

More information

Candidate Style Answer

Candidate Style Answer Candidate Style Answer Chemistry A Unit F321 Atoms, Bonds and Groups High banded response This Support Material booklet is designed to accompany the OCR GCE Chemistry A Specimen Paper F321 for teaching

More information

Name Class Date. What is ionic bonding? What happens to atoms that gain or lose electrons? What kinds of solids are formed from ionic bonds?

Name Class Date. What is ionic bonding? What happens to atoms that gain or lose electrons? What kinds of solids are formed from ionic bonds? CHAPTER 1 2 Ionic Bonds SECTION Chemical Bonding BEFORE YOU READ After you read this section, you should be able to answer these questions: What is ionic bonding? What happens to atoms that gain or lose

More information

Part I: Principal Energy Levels and Sublevels

Part I: Principal Energy Levels and Sublevels Part I: Principal Energy Levels and Sublevels As you already know, all atoms are made of subatomic particles, including protons, neutrons, and electrons. Positive protons and neutral neutrons are found

More information

Electrons in Atoms & Periodic Table Chapter 13 & 14 Assignment & Problem Set

Electrons in Atoms & Periodic Table Chapter 13 & 14 Assignment & Problem Set Electrons in Atoms & Periodic Table Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. Electrons in Atoms & Periodic Table 2 Study Guide: Things You

More information

Honors Chemistry: Unit 6 Test Stoichiometry PRACTICE TEST ANSWER KEY Page 1. A chemical equation. (C-4.4)

Honors Chemistry: Unit 6 Test Stoichiometry PRACTICE TEST ANSWER KEY Page 1. A chemical equation. (C-4.4) Honors Chemistry: Unit 6 Test Stoichiometry PRACTICE TEST ANSWER KEY Page 1 1. 2. 3. 4. 5. 6. Question What is a symbolic representation of a chemical reaction? What 3 things (values) is a mole of a chemical

More information

CHEMISTRY BONDING REVIEW

CHEMISTRY BONDING REVIEW Answer the following questions. CHEMISTRY BONDING REVIEW 1. What are the three kinds of bonds which can form between atoms? The three types of Bonds are Covalent, Ionic and Metallic. Name Date Block 2.

More information

19.2 Chemical Formulas

19.2 Chemical Formulas In the previous section, you learned how and why atoms form chemical bonds with one another. You also know that atoms combine in certain ratios with other atoms. These ratios determine the chemical formula

More information

SCPS Chemistry Worksheet Periodicity A. Periodic table 1. Which are metals? Circle your answers: C, Na, F, Cs, Ba, Ni

SCPS Chemistry Worksheet Periodicity A. Periodic table 1. Which are metals? Circle your answers: C, Na, F, Cs, Ba, Ni SCPS Chemistry Worksheet Periodicity A. Periodic table 1. Which are metals? Circle your answers: C, Na, F, Cs, Ba, Ni Which metal in the list above has the most metallic character? Explain. Cesium as the

More information

Atomic Structure. Name Mass Charge Location Protons 1 +1 Nucleus Neutrons 1 0 Nucleus Electrons 1/1837-1 Orbit nucleus in outer shells

Atomic Structure. Name Mass Charge Location Protons 1 +1 Nucleus Neutrons 1 0 Nucleus Electrons 1/1837-1 Orbit nucleus in outer shells Atomic Structure called nucleons Name Mass Charge Location Protons 1 +1 Nucleus Neutrons 1 0 Nucleus Electrons 1/1837-1 Orbit nucleus in outer shells The number of protons equals the atomic number This

More information

Which substance contains positive ions immersed in a sea of mobile electrons? A) O2(s) B) Cu(s) C) CuO(s) D) SiO2(s)

Which substance contains positive ions immersed in a sea of mobile electrons? A) O2(s) B) Cu(s) C) CuO(s) D) SiO2(s) BONDING MIDTERM REVIEW 7546-1 - Page 1 1) Which substance contains positive ions immersed in a sea of mobile electrons? A) O2(s) B) Cu(s) C) CuO(s) D) SiO2(s) 2) The bond between hydrogen and oxygen in

More information

Elements, Atoms & Ions

Elements, Atoms & Ions Introductory Chemistry: A Foundation FOURTH EDITION by Steven S. Zumdahl University of Illinois Elements, Atoms & Ions Chapter 4 1 2 Elements Aims: To learn about the relative abundances of the elements,

More information

WRITING CHEMICAL FORMULA

WRITING CHEMICAL FORMULA WRITING CHEMICAL FORMULA For ionic compounds, the chemical formula must be worked out. You will no longer have the list of ions in the exam (like at GCSE). Instead you must learn some and work out others.

More information

EXPERIMENT 4 The Periodic Table - Atoms and Elements

EXPERIMENT 4 The Periodic Table - Atoms and Elements EXPERIMENT 4 The Periodic Table - Atoms and Elements INTRODUCTION Primary substances, called elements, build all the materials around you. There are more than 109 different elements known today. The elements

More information

CHEMICAL FORMULAS AND EQUATIONS

CHEMICAL FORMULAS AND EQUATIONS reflect Imagine that you and three other classmates had enough supplies and the recipe to make one pepperoni pizza. The recipe might include a ball of dough, a cup of pizza sauce, a cup of cheese, and

More information

Exam 2 Chemistry 65 Summer 2015. Score:

Exam 2 Chemistry 65 Summer 2015. Score: Name: Exam 2 Chemistry 65 Summer 2015 Score: Instructions: Clearly circle the one best answer 1. Valence electrons are electrons located A) in the outermost energy level of an atom. B) in the nucleus of

More information

5.4 Trends in the Periodic Table

5.4 Trends in the Periodic Table 5.4 Trends in the Periodic Table Think about all the things that change over time or in a predictable way. For example, the size of the computer has continually decreased over time. You may become more

More information

Chapter 6 Assessment. Name: Class: Date: ID: A. Multiple Choice Identify the choice that best completes the statement or answers the question.

Chapter 6 Assessment. Name: Class: Date: ID: A. Multiple Choice Identify the choice that best completes the statement or answers the question. Name: Class: Date: ID: A Chapter 6 Assessment Multiple Choice Identify the choice that best completes the statement or answers the question. 1. When an atom loses an electron, it forms a(n) a. anion. c.

More information

Sample Exercise 2.1 Illustrating the Size of an Atom

Sample Exercise 2.1 Illustrating the Size of an Atom Sample Exercise 2.1 Illustrating the Size of an Atom The diameter of a US penny is 19 mm. The diameter of a silver atom, by comparison, is only 2.88 Å. How many silver atoms could be arranged side by side

More information

Objectives. PAM1014 Introduction to Radiation Physics. Constituents of Atoms. Atoms. Atoms. Atoms. Basic Atomic Theory

Objectives. PAM1014 Introduction to Radiation Physics. Constituents of Atoms. Atoms. Atoms. Atoms. Basic Atomic Theory PAM1014 Introduction to Radiation Physics Basic Atomic Theory Objectives Introduce and Molecules The periodic Table Electronic Energy Levels Atomic excitation & de-excitation Ionisation Molecules Constituents

More information

PERIODIC TABLE OF GROUPS OF ELEMENTS Elements can be classified using two different schemes.

PERIODIC TABLE OF GROUPS OF ELEMENTS Elements can be classified using two different schemes. 1 PERIODIC TABLE OF GROUPS OF ELEMENTS Elements can be classified using two different schemes. Metal Nonmetal Scheme (based on physical properties) Metals - most elements are metals - elements on left

More information

Chemistry Post-Enrolment Worksheet

Chemistry Post-Enrolment Worksheet Name: Chemistry Post-Enrolment Worksheet The purpose of this worksheet is to get you to recap some of the fundamental concepts that you studied at GCSE and introduce some of the concepts that will be part

More information

Instructors Guide: Atoms and Their Isotopes

Instructors Guide: Atoms and Their Isotopes Instructors Guide: Atoms and Their Isotopes Standards Connections Connections to NSTA Standards for Science Teacher Preparation C.3.a.1 Fundamental structures of atoms and molecules. C.3.b.27 Applications

More information

9/13/2013. However, Dalton thought that an atom was just a tiny sphere with no internal parts. This is sometimes referred to as the cannonball model.

9/13/2013. However, Dalton thought that an atom was just a tiny sphere with no internal parts. This is sometimes referred to as the cannonball model. John Dalton was an English scientist who lived in the early 1800s. Dalton s atomic theory served as a model for how matter worked. The principles of Dalton s atomic theory are: 1. Elements are made of

More information

Theme 3: Bonding and Molecular Structure. (Chapter 8)

Theme 3: Bonding and Molecular Structure. (Chapter 8) Theme 3: Bonding and Molecular Structure. (Chapter 8) End of Chapter questions: 5, 7, 9, 12, 15, 18, 23, 27, 28, 32, 33, 39, 43, 46, 67, 77 Chemical reaction valence electrons of atoms rearranged (lost,

More information

Unit 1 Chemical Changes and Structure Revision Notes

Unit 1 Chemical Changes and Structure Revision Notes Unit 1 Revision Notes Rates of reaction The rate of reaction can be increased by: increasing the concentration of a solution decreasing the particle size of a solid increasing the temperature adding a

More information

Chemistry Diagnostic Questions

Chemistry Diagnostic Questions Chemistry Diagnostic Questions Answer these 40 multiple choice questions and then check your answers, located at the end of this document. If you correctly answered less than 25 questions, you need to

More information

2014 Spring CHEM101 Ch1-2 Review Worksheet Modified by Dr. Cheng-Yu Lai,

2014 Spring CHEM101 Ch1-2 Review Worksheet Modified by Dr. Cheng-Yu Lai, Ch1 1) Which of the following underlined items is not an intensive property? A) A chemical reaction requires 3.00 g of oxygen. B) The density of helium at 25 C is 1.64 10-4 g/cm3. C) The melting point

More information

Name period AP chemistry Unit 2 worksheet Practice problems

Name period AP chemistry Unit 2 worksheet Practice problems Name period AP chemistry Unit 2 worksheet Practice problems 1. What are the SI units for a. Wavelength of light b. frequency of light c. speed of light Meter hertz (s -1 ) m s -1 (m/s) 2. T/F (correct

More information

Chapter 1: Moles and equations. Learning outcomes. you should be able to:

Chapter 1: Moles and equations. Learning outcomes. you should be able to: Chapter 1: Moles and equations 1 Learning outcomes you should be able to: define and use the terms: relative atomic mass, isotopic mass and formula mass based on the 12 C scale perform calculations, including

More information

Chapter 2 Atoms, Molecules, and Ions

Chapter 2 Atoms, Molecules, and Ions Chapter 2 Atoms, Molecules, and Ions 1. Methane and ethane are both made up of carbon and hydrogen. In methane, there are 12.0 g of carbon for every 4.00 g of hydrogen, a ration of 3:1 by mass. In ethane,

More information

LEWIS DIAGRAMS. by DR. STEPHEN THOMPSON MR. JOE STALEY

LEWIS DIAGRAMS. by DR. STEPHEN THOMPSON MR. JOE STALEY by DR. STEPHEN THOMPSON MR. JOE STALEY The contents of this module were developed under grant award # P116B-001338 from the Fund for the Improvement of Postsecondary Education (FIPSE), United States Department

More information

Stoichiometry Review

Stoichiometry Review Stoichiometry Review There are 20 problems in this review set. Answers, including problem set-up, can be found in the second half of this document. 1. N 2 (g) + 3H 2 (g) --------> 2NH 3 (g) a. nitrogen

More information

ATOMS. Multiple Choice Questions

ATOMS. Multiple Choice Questions Chapter 3 ATOMS AND MOLECULES Multiple Choice Questions 1. Which of the following correctly represents 360 g of water? (i) 2 moles of H 2 0 (ii) 20 moles of water (iii) 6.022 10 23 molecules of water (iv)

More information

TOPIC 7. CHEMICAL CALCULATIONS I - atomic and formula weights.

TOPIC 7. CHEMICAL CALCULATIONS I - atomic and formula weights. TOPIC 7. CHEMICAL CALCULATIONS I - atomic and formula weights. Atomic structure revisited. In Topic 2, atoms were described as ranging from the simplest atom, H, containing a single proton and usually

More information

MOLES AND MOLE CALCULATIONS

MOLES AND MOLE CALCULATIONS 35 MOLES ND MOLE CLCULTIONS INTRODUCTION The purpose of this section is to present some methods for calculating both how much of each reactant is used in a chemical reaction, and how much of each product

More information

2. John Dalton did his research work in which of the following countries? a. France b. Greece c. Russia d. England

2. John Dalton did his research work in which of the following countries? a. France b. Greece c. Russia d. England CHAPTER 3 1. Which combination of individual and contribution is not correct? a. Antoine Lavoisier - clarified confusion over cause of burning b. John Dalton - proposed atomic theory c. Marie Curie - discovered

More information

In the box below, draw the Lewis electron-dot structure for the compound formed from magnesium and oxygen. [Include any charges or partial charges.

In the box below, draw the Lewis electron-dot structure for the compound formed from magnesium and oxygen. [Include any charges or partial charges. Name: 1) Which molecule is nonpolar and has a symmetrical shape? A) NH3 B) H2O C) HCl D) CH4 7222-1 - Page 1 2) When ammonium chloride crystals are dissolved in water, the temperature of the water decreases.

More information

Ions & Their Charges Worksheet

Ions & Their Charges Worksheet Ions & Their Charges Worksheet Name Date Teacher Diagram of charges based on groups on the periodic table including transition metals and noble gases: IA IIA Transition IIIA IVA VA VIA VIIA VIIIA metals

More information

Element of same atomic number, but different atomic mass o Example: Hydrogen

Element of same atomic number, but different atomic mass o Example: Hydrogen Atomic mass: p + = protons; e - = electrons; n 0 = neutrons p + + n 0 = atomic mass o For carbon-12, 6p + + 6n 0 = atomic mass of 12.0 o For chlorine-35, 17p + + 18n 0 = atomic mass of 35.0 atomic mass

More information

Chemistry CP Unit 2 Atomic Structure and Electron Configuration. Learning Targets (Your exam at the end of Unit 2 will assess the following:)

Chemistry CP Unit 2 Atomic Structure and Electron Configuration. Learning Targets (Your exam at the end of Unit 2 will assess the following:) Chemistry CP Unit 2 Atomic Structure and Electron Learning Targets (Your exam at the end of Unit 2 will assess the following:) 2. Atomic Structure and Electron 2-1. Give the one main contribution to the

More information

Electron Configurations, Isoelectronic Elements, & Ionization Reactions. Chemistry 11

Electron Configurations, Isoelectronic Elements, & Ionization Reactions. Chemistry 11 Electron Configurations, Isoelectronic Elements, & Ionization Reactions Chemistry 11 Note: Of the 3 subatomic particles, the electron plays the greatest role in determining the physical and chemical properties

More information

Composition of nucleus. Priority Vocabulary: Electron, Proton, Neutron, Nucleus, Isotopes, Atomic Number, Atomic Mass, Element, Electron Shell,

Composition of nucleus. Priority Vocabulary: Electron, Proton, Neutron, Nucleus, Isotopes, Atomic Number, Atomic Mass, Element, Electron Shell, Lake County, Lakeview, 9 th grade, Physical Science, Brent Starr Standard: H1P1 Explain how atomic structure is related to the properties of elements and their position in the Periodic Table. Explain how

More information

Chemical Equations and Chemical Reactions. Chapter 8.1

Chemical Equations and Chemical Reactions. Chapter 8.1 Chemical Equations and Chemical Reactions Chapter 8.1 Objectives List observations that suggest that a chemical reaction has taken place List the requirements for a correctly written chemical equation.

More information

Science 20. Unit A: Chemical Change. Assignment Booklet A1

Science 20. Unit A: Chemical Change. Assignment Booklet A1 Science 20 Unit A: Chemical Change Assignment Booklet A FOR TEACHER S USE ONLY Summary Teacher s Comments Chapter Assignment Total Possible Marks 79 Your Mark Science 20 Unit A: Chemical Change Assignment

More information

The Periodic Table: Periodic trends

The Periodic Table: Periodic trends Unit 1 The Periodic Table: Periodic trends There are over one hundred different chemical elements. Some of these elements are familiar to you such as hydrogen, oxygen, nitrogen and carbon. Each one has

More information

3. What would you predict for the intensity and binding energy for the 3p orbital for that of sulfur?

3. What would you predict for the intensity and binding energy for the 3p orbital for that of sulfur? PSI AP Chemistry Periodic Trends MC Review Name Periodic Law and the Quantum Model Use the PES spectrum of Phosphorus below to answer questions 1-3. 1. Which peak corresponds to the 1s orbital? (A) 1.06

More information

CHEMICAL NAMES AND FORMULAS

CHEMICAL NAMES AND FORMULAS 6 CEMICAL NAMES AND FORMULAS SECTION 6.1 INTRODUCTION TO CEMICAL BONDING (pages 133 137) This section explains how to distinguish between ionic and molecular compounds. It also defines cation and anion

More information

Calculating Atoms, Ions, or Molecules Using Moles

Calculating Atoms, Ions, or Molecules Using Moles TEKS REVIEW 8B Calculating Atoms, Ions, or Molecules Using Moles TEKS 8B READINESS Use the mole concept to calculate the number of atoms, ions, or molecules in a sample TEKS_TXT of material. Vocabulary

More information

Unit 6 The Mole Concept

Unit 6 The Mole Concept Chemistry Form 3 Page 62 Ms. R. Buttigieg Unit 6 The Mole Concept See Chemistry for You Chapter 28 pg. 352-363 See GCSE Chemistry Chapter 5 pg. 70-79 6.1 Relative atomic mass. The relative atomic mass

More information

IB Chemistry 1 Mole. One atom of C-12 has a mass of 12 amu. One mole of C-12 has a mass of 12 g. Grams we can use more easily.

IB Chemistry 1 Mole. One atom of C-12 has a mass of 12 amu. One mole of C-12 has a mass of 12 g. Grams we can use more easily. The Mole Atomic mass units and atoms are not convenient units to work with. The concept of the mole was invented. This was the number of atoms of carbon-12 that were needed to make 12 g of carbon. 1 mole

More information

Matter. Atomic weight, Molecular weight and Mole

Matter. Atomic weight, Molecular weight and Mole Matter Atomic weight, Molecular weight and Mole Atomic Mass Unit Chemists of the nineteenth century realized that, in order to measure the mass of an atomic particle, it was useless to use the standard

More information

Word Equations and Balancing Equations. Video Notes

Word Equations and Balancing Equations. Video Notes Word Equations and Balancing Equations Video Notes In this lesson, you will: Use the law of conservation of mass and provide standard rules for writing and balancing equations. Write and balance equations

More information

Chapter 8 Basic Concepts of the Chemical Bonding

Chapter 8 Basic Concepts of the Chemical Bonding Chapter 8 Basic Concepts of the Chemical Bonding 1. There are paired and unpaired electrons in the Lewis symbol for a phosphorus atom. (a). 4, 2 (b). 2, 4 (c). 4, 3 (d). 2, 3 Explanation: Read the question

More information

Amount of Substance. http://www.avogadro.co.uk/definitions/elemcompmix.htm

Amount of Substance. http://www.avogadro.co.uk/definitions/elemcompmix.htm Page 1 of 14 Amount of Substance Key terms in this chapter are: Element Compound Mixture Atom Molecule Ion Relative Atomic Mass Avogadro constant Mole Isotope Relative Isotopic Mass Relative Molecular

More information

PERIODIC TABLE. reflect

PERIODIC TABLE. reflect reflect Suppose you wanted to organize your locker at school. How could you separate and arrange everything in an organized way? You could place the books, notebooks, and folders on a shelf that is separate

More information

Name: Worksheet: Electron Configurations. I Heart Chemistry!

Name: Worksheet: Electron Configurations. I Heart Chemistry! 1. Which electron configuration represents an atom in an excited state? 1s 2 2s 2 2p 6 3p 1 1s 2 2s 2 2p 6 3s 2 3p 2 1s 2 2s 2 2p 6 3s 2 3p 1 1s 2 2s 2 2p 6 3s 2 Worksheet: Electron Configurations Name:

More information

TRENDS IN THE PERIODIC TABLE

TRENDS IN THE PERIODIC TABLE Noble gases Period alogens Alkaline earth metals Alkali metals TRENDS IN TE PERIDI TABLE Usual charge +1 + +3-3 - -1 Number of Valence e - s 1 3 4 5 6 7 Electron dot diagram X X X X X X X X X 8 Group 1

More information

Chapter Five: Atomic Theory and Structure

Chapter Five: Atomic Theory and Structure Chapter Five: Atomic Theory and Structure Evolution of Atomic Theory The ancient Greek scientist Democritus is often credited with developing the idea of the atom Democritus proposed that matter was, on

More information

Chapter Outline. 3 Elements and Compounds. Elements and Atoms. Elements. Elements. Elements 9/4/2013

Chapter Outline. 3 Elements and Compounds. Elements and Atoms. Elements. Elements. Elements 9/4/2013 3 Elements and Compounds Chapter Outline 3.1 Elements A. Distribution of Elements Foundations of College Chemistry, 14 th Ed. Morris Hein and Susan Arena Copyright This reclining Buddha in Thailand is

More information

ANSWER KEY. Energy Levels, Electrons and IONIC Bonding It s all about the Give and Take!

ANSWER KEY. Energy Levels, Electrons and IONIC Bonding It s all about the Give and Take! ANSWER KEY Energy Levels, Electrons and IONIC Bonding It s all about the Give and Take! From American Chemical Society Middle School Chemistry Unit: Chapter 4 Content Statements: Distinguish the difference

More information

Chapter 7 Periodic Properties of the Elements

Chapter 7 Periodic Properties of the Elements Chapter 7 Periodic Properties of the Elements 1. Elements in the modern version of the periodic table are arranged in order of increasing. (a). oxidation number (b). atomic mass (c). average atomic mass

More information