Question Bank Atomic Structure

Save this PDF as:
 WORD  PNG  TXT  JPG

Size: px
Start display at page:

Download "Question Bank Atomic Structure"

Transcription

1 Atomic Structure 1. An atom is made of charged particles called protons and electrons. Why is an atom uncharged? Ans. In an atom (i) the number of electrons is equal to the number of protons. (ii) the total negative charge on the electrons is equal to the total positive charge on the protons. Thus, an atom is electrically neutral. 2. (a) An atom usually contains three particles. Name the particles and state the charge they carry and their relative masses with respect to hydrogen. (b) Which element contains only two of these types of particles in its atom? Ans. (a) The particles are electrons, protons and neutrons. The mass of an electron is hydrogen or times the atomic mass of The charge is 1 elementary charge unit. The mass of a proton is equal to the atomic mass unit of hydrogen and charge is equal to +1 elementary charge unit. The mass of neutron is equal to the atomic mass unit of hydrogen, but it has no electric charge. (b) Hydrogen : It has one proton and one electron. 1

2 3. What is meant by the following statements : (i) Atomic number of calcium is 20? (ii) Mass number of calcium is 40? Ans. (i) It means the nucleus of calcium has 20 protons and hence it has a charge +20 elementary charge units. Furthermore, there are 20 electrons revolving around the nucleus of calcium. (ii) It means the total number of protons and neutrons (each having a mass equivalent to 1 a.m.u) are 40 in the nucleus of calcium. 4. What is meant by the statement that atomic number of sodium is 11? Ans. It means : (i) There are 11 protons in the nucleus of sodium. (ii) The total atomic mass of protons is 11 a.m.u. (iii) The total elementary charge is +11 units. (iv) The total number of electrons revolving around the nucleus of sodium is What do you understand by the term electronic configuration? Write down the electronic configuration of the following elements. (i) Magnesium (At. No. 12). (ii) Chlorine (At. No. 17). Ans. Electronic configuration : The arrangement of electrons into various energy levels around the nucleus of an atom is called electronic configuration. Electronic configuration of magnesium is K L M Electronic configuration of chlorine is K L M

3 6. Write down the names of the following particles and explain the meaning of their symbol, superscript, subscript, where P stands for the particle p; 0 p; 1p Ans. 1 1 p Particle is proton. Superscript denotes its mass is 1 a.m.u p Subscript denotes its elementary charge is +1 unit. 1 0 p Particle is neutron. Superscript denotes its mass is 1 a.m.u Subscript denotes its charge is zero. 0 1 Particle is electron. Superscript denotes its mass is 0 (zero) a.m.u, i.e., it has no mass. Subscript denotes its elementary charge is 1 unit. 7. An atom of fluorine may be written as Write down : (1) the number of protons. (2) the number of neutrons. (3) the number of electrons in an atom of fluorine. Show the atom by geometric diagram. Ans. 19 No. of protons = 9 9 F No. of neutrons = Z A = 19 9 = 10 No. of electrons = 9 (2,7). Geometric representation of fluorine atom. 3

4 24 8. From the symbol 12 Mg state : (i) its mass number, (ii)its atomic number, Ans. (i) Mass number is 24. (iii) its electronic configuration. (ii) Atomic number is 12. (iii) Electronic configuration : K (2), L(8), M(2) Draw the structures of (i) Sodium atom Na (ii) fluorine atom 19 F Ans. (i) (ii) 10. Structure of Na Structure of 19 9 F Element Mass No. Atomic No. Number of protons Number of neutrons Potassium Cl Cl (a) Complete the table given above. (b) What is the name given to the pair of atoms, such as Cl and 37 Cl 17 17? 4

5 Ans. (a) Element Mass No. Atomic No. Number of protons Number of neutrons Potassium = Cl = Cl = 20 (b) The pair of atoms and 37 17Cl 17 Cl are called isotopes. 11. By using isotopes of chlorine and 37 17Cl 17 Cl, give reasons (or explain): (i) Two isotopes have identical properties. (ii) The relative mass of chlorine is not a whole number. 17 Cl Cl Ans.(i) and have the same number of protons and hence electrons. Thus, they have the same electronic configuration, i.e., same number of electrons in the valence shell. It is on account of the same number of electrons in their valence shell, that they have similar chemical properties. 17 Cl Cl (ii) Natural chlorine contains isotopes and in the ratio of 3:1. Thus, their relative atomic mass is an average of the atomic masses of the isotopes and hence it is not a whole number (a) Three different atoms of hydrogen are represented as 1 H, 2 H, H. What do the subscripts and superscripts represent? (b) Which factor is responsible for the change in the superscripts, 1, 2 and 3 though the element is the same? 5

6 (c) What is the appropriate term for the elements having such a property? (d) Draw the atomic structure of 3 1 H. Ans.(a) The superscripts represent mass number The subscripts represent atomic number. (b) It is the excess neutrons, which are responsible for the change in mass number. In 1 2 1H there is no neutron, in there is one neutron and in 3 1 H 1 H there are two neutrons in the nucleus of hydrogen. (c) Isotopes is the appropriate term. (d) Structure of 3 1 H is as shown alongside. 24 Mg and 12Mg are the symbols of two isotopes of magnesium. Compare the atoms of these isotopes with respect to : (i) Composition of their nuclei. (ii) Electronic configuration. (iii) Give reason why the two isotopes of magnesium have different mass numbers. Ans. (i) The nucleus of Mg has 12 protons and 14 neutrons. The nucleus of Mg has 12 protons and 12 neutrons. (ii) Electronic configuration of Mg and 12 Mg is K L M

7 26 (iii) The difference in the mass number is due to two extra neutrons in 12 Mg. 14. Chlorine is an element with atomic number 17. It is a mixture of two isotopes of mass number and 37 in the ratio of 3:1. (i) What is meant by the atomic number of an element? (ii) Write down the electronic configuration of chlorine. (iii) Calculate the average relative mass of chlorine. Ans. (i) The number of protons present in the nucleus of an atom is called its atomic number. (ii) The electronic configuration of chlorine is K L M (iii) Relative atomic mass of chlorine Ar = xa + ya x + y 1 2 = = 37 = 142 = Calculate the relative atomic masses of the following elements : (a) Copper, which consists of 69% of copper 63 and 31% of copper 65. (b) Gallium, which consists of 60% of Gallium 69 and 40% of Gallium 71. Ans. (a) Relative atomic mass of copper Ar = xa + ya 1 2 x + y =

8 (b)relative atomic mass of Gallium Ar = = = = = xa1 + ya = x+ y = = Write the symbols with mass number and atomic number of the following: (a) Arsenic (atomic number 33, mass number 75). (b) Uranium 238(atomic number 92). (c) Uranium 2(atomic number 92). (d) Uranium 239(atomic number 92). Ans. (a) Arsenic [At. No. 33, Mass No. 75] As (b) Uranium [At. No. 92, Mass No. 238] U (c) Uranium [At. No. 92, Mass No. 2] 2 92 U (d) Uranium [At. No. 92, Mass No. 239] U 17. Complete the following table : Element Mass No. Atomic No. Neutrons Protons Electrons Electronic configuration Carbon Aluminium Fluorine , 7 Argon Helium Sodium

9 Ans. Element Mass No. At. No. Neutrons Protons Electrons Electronic configuration K, L, M Carbon , 4 Aluminium , 8, 3 Flourine , 7 Argon , 8, 8 Helium Sodium , 8, (i) What do you understand by the term valence electrons? (ii) Why are valence electrons named as such, rather than only electrons? Ans. (i) The electrons present in the outermost shell of an atom are called valence electrons. (ii) They are named as valence electrons, because it is these electrons which take part in a chemical reaction either by actual transfer or by sharing. 19. An element is represented as X. Name the shell which has valence electrons and the number of valence electrons in it. Ans. Electronic configuration of 40 X 20 is 2(K), 8(L), 8(M), 2(N). The valence shell is the N-shell. It has 2 valence electrons. 9

10 20. Amongst the electrons revolving around the nucleus, which electrons (i) determine the chemical properties of an element, (ii) do not determine the chemical properties of an element? Give reasons for your answer. Ans. (i) The electrons in the valence shell determine the chemical properties of an element. (ii) The electrons other than the electrons in the valence shell, do not determine the chemical properties of an element. Reason : The electrons in the valence shell are weakly held by the nucleus. Thus, an element can donate or accept or share these electrons with the atoms of other elements and hence enters into a chemical reaction. 21. Fill in the blank spaces with appropriate words : (i) The electrons present in the (1) shell of an atom are called valence electrons. (ii) The electrons present in a shell, other than the (2) shell do not take part in a (3) reaction. (iii) The nature of an element is (4), if it has one to three (5) electrons. (iv) The element is a (6) gas, if it has (7) valence electrons. (v) The element (8) has one electron in the K-shell, but is a non-metal. 10

11 (vi)the element (9) has two electrons in the K-shell, but is a noble gas. Ans. (1) valence (2) valence (3) chemical (4) metallic (5) valence (6) noble (7) eight (8) hydrogen (9) helium. 21. Elements A, B and C have atomic numbers 9, 20 and 10 respectively. State which one is : (a) metal, (b) non-metal, (c) inert gas? Ans. Electronic configuration of A(9) is (2, 7). As there are 7 electrons in the valence shell, hence A is a non- metal. Electronic configuration of B(20) is (2, 8, 8, 2). As there are 2 electrons in the valence shell, hence B is a metal. Electronic configuration of C(10) is (2, 8). As there are 8 electrons in the valence shell, hence C is an inert gas. 22. A, B, C and D are the elements whose atomic numbers are 16,19,18 and 13 respectively. Write down the electronic configuration of each element and classify them as metal/non-metal/ noble gas. Ans. A (atomic no. 16) has electronic configuration of (2, 8, 6) and hence is a non-metal. B (atomic no. 19) has electronic configuration of (2, 8, 8, 1) and hence is a metal. 11

12 C (atomic no. 18] has electronic configuration of (2, 8, 8) and hence is a noble gas. D (atomic no. 13] has electronic configuration of (2, 8, 3) and hence is a metal. 23. Complete the table below, with the elements E, F, G, H, such that element E is an inert gas having electronic configuration 2,8. Ans. Elements Atomic number Electronic configuration E Z 2, 8 F Z G Z H Z Which of the elements in the table are (i) metals,(ii) non-metals? Elements Atomic number Electronic configuration E Z 2, 8 F Z 1 2, 7 G Z + 1 2, 8, 1 H Z + 4 2, 8, 4 (i) G is a metal. (ii) F and H are non-metals. 12

13 24. Which of the following elements would you expect to be most stable and why? A, 13B, 11C, 18D Ans. Elements 4 2A [2(K)] and D they have 2 and 8 electrons in their valence shell. [2(K), 8(L), 8(M)] are most stable, because 13

1. Structure and Properties of the Atom

1. Structure and Properties of the Atom SACE Stage 1 Chemistry - The Essentials 1. Structure and Properties of the Atom 1.1 Atoms: A simple definition of the atom is that it is the smallest particle that contains the properties of that element.

More information

The Atom Atomic Number Mass Number Isotopes

The Atom Atomic Number Mass Number Isotopes The Atom Atomic Number Mass Number Isotopes 1 Atomic Theory Atoms are building blocks of elements Similar atoms in each element Different from atoms of other elements Two or more different atoms bond in

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

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

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

Atomic Theory and Bonding

Atomic Theory and Bonding Atomic Theory and Bonding Textbook pages 168 183 Section 4.1 Summary Before You Read What do you already know about Bohr diagrams? Record your answer in the lines below. What are atoms? An atom is the

More information

Matter, Elements, Compounds, Chemical Bonds and Energy

Matter, Elements, Compounds, Chemical Bonds and Energy Science of Kriyayoga IST 111-01, Spring 2005 Matter, Elements, Compounds, Chemical Bonds and Energy In our discussion so far, we have discussed human nervous system and cell biology, in addition to the

More information

2. All of the atoms of argon have the same. 1. The atomic number of an atom is always equal to the total number of. A. mass number B.

2. All of the atoms of argon have the same. 1. The atomic number of an atom is always equal to the total number of. A. mass number B. 1. The atomic number of an atom is always equal to the total number of A. neutrons in the nucleus B. protons in the nucleus 2. All of the atoms of argon have the same A. mass number B. atomic number C.

More information

Science and technology 404

Science and technology 404 Name Date STUDY GUIDE CHAPTER 1 ATOMS AND ELEMENTS 1) DESCRIBE THE RUTHERFORD-BOHR ATOMIC MODEL All matter is made of small particles called atoms. An atom is the smallest unit of matter that retains the

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

1. According to the modern model of the atom, the nucleus of an atom is surrounded by one or more

1. According to the modern model of the atom, the nucleus of an atom is surrounded by one or more 1. According to the modern model of the atom, the nucleus of an atom is surrounded by one or more 8. The diagram below represents the nucleus of an atom. A) electrons B) neutrons C) positrons D) protons

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

( + and - ) ( - and - ) ( + and + ) Atoms are mostly empty space. = the # of protons in the nucleus. = the # of protons in the nucleus

( + and - ) ( - and - ) ( + and + ) Atoms are mostly empty space. = the # of protons in the nucleus. = the # of protons in the nucleus Atoms are mostly empty space Atomic Structure Two regions of every atom: Nucleus - is made of protons and neutrons - is small and dense Electron cloud -is a region where you might find an electron -is

More information

Unit 2: Atomic Theory Practice Packet

Unit 2: Atomic Theory Practice Packet Unit 2: Atomic Theory Practice Packet 1 Name History of Atomic Theory Period Fill in the missing information in the chart below: Name of Researcher Equipment Sketch of Model Major Idea/Discovery N/A All

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

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

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

ATOMIC THEORY. Name Symbol Mass (approx.; kg) Charge

ATOMIC THEORY. Name Symbol Mass (approx.; kg) Charge ATOMIC THEORY The smallest component of an element that uniquely defines the identity of that element is called an atom. Individual atoms are extremely small. It would take about fifty million atoms in

More information

Atomic Structure. Atoms and elements

Atomic Structure. Atoms and elements Atomic Structure Atoms and elements Everything in the world is made up from about 100 elements. Every element is made up of very small particles called atoms. An element is a substance in which all the

More information

Test 2: Atomic Structure Review

Test 2: Atomic Structure Review Name: Monday, October 15, 2007 Test 2: Atomic Structure Review 1. Figure 1 The diagram shows the characteristic spectral line patterns of four elements. Also shown are spectral lines produced by an unknown

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

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

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

Atomic Theory: The Nuclear Model of the Atom

Atomic Theory: The Nuclear Model of the Atom Chapter 5 Atomic Theory: The Nuclear Model of the Atom Section 5.1 Dalton s Atomic Theory Goal 1 Precursors to John Dalton s atomic theory Law of Definite Composition The percentage by mass of the elements

More information

Short questions: Write the nuclear symbols for three isotopes of oxygen in which there are 8, 9, and 10 neutrons, respectively.

Short questions: Write the nuclear symbols for three isotopes of oxygen in which there are 8, 9, and 10 neutrons, respectively. Atom X A Z A mass number (= number of protons (electrons) + number of neutrons) Z atomic number (= number of protons = number of electrons) Almost all of the mass of an atom is in its nucleus; almost all

More information

Multiple Choice Questions

Multiple Choice Questions Chapter 4 STRUCTURE OF THE ATOM Multiple Choice Questions 1. Which of the following correctly represent the electronic distribution in the Mg atom? 3, 8, 1 (b) 2, 8, 2 (c) 1, 8, 3 (d) 8, 2, 2 2. Rutherford

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

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

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

Composition and Structure of the Atom. Protons: Positively charged, high mass particle. Neutrons: Neutral (no) charge, high mass

Composition and Structure of the Atom. Protons: Positively charged, high mass particle. Neutrons: Neutral (no) charge, high mass Composition and Structure of the Atom Atom: basic unit of an element; smallest unit that retains chemical properties of an element Subatomic particles: Small particles that are the building blocks from

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

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

Atoms, Isotopes, and Ions

Atoms, Isotopes, and Ions WHY? ACTIVITY 02-1 Atoms, Isotopes, and Ions Atoms are the fundamental building blocks of all substances. To begin to understand the properties of atoms and how they combine to form molecules, you must

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

Atoms, Molecules, Formulas, and Subatomic Particles

Atoms, Molecules, Formulas, and Subatomic Particles Introduction to Chemistry Chapter 5 1 Atoms, Molecules, Formulas, and Subatomic Particles The Atom: The smallest particle of an element that can exist and still have the properties of the element building

More information

Chapter 3 Atoms & the. Chapter 3 Section 2 The Simplest Matter Pages 80-85

Chapter 3 Atoms & the. Chapter 3 Section 2 The Simplest Matter Pages 80-85 Chapter 3 Atoms & the Periodic Table Chapter 3 Section 2 The Simplest Matter Pages 80-85 The Elements There are many different types of atoms. An element is matter made up of only one kind of atom. An

More information

Name. Worksheet: Periodic Trends. 11. Which sequence of elements is arranged in order of decreasing atomic radii?

Name. Worksheet: Periodic Trends. 11. Which sequence of elements is arranged in order of decreasing atomic radii? 1. Which statement best describes Group 2 elements as they are considered in order from top to bottom of the Periodic Table? (A) The number of principal energy levels increases, and the number of valence

More information

Atomic Concepts Review

Atomic Concepts Review 1. Which phrase describes an atom? A) a negatively charged nucleus surrounded by positively charged protons B) a negatively charged nucleus surrounded by positively charged electrons C) a positively charged

More information

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

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

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

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

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

Explain 'Dobereiner's Triads and its drawback.

Explain 'Dobereiner's Triads and its drawback. CLASS: X NCERT (CBSE) Chemistry: For Class 10 Page : 1 Question 1: Explain 'Dobereiner's Triads and its drawback. Dobereiner classified elements into groups of three where the atomic weight of the middle

More information

Period 3 elements

Period 3 elements 3.1.4.2 Period 3 elements 173 minutes 169 marks Page 1 of 17 Q1. (a) Explain why certain elements in the Periodic Table are classified as p-block elements. Illustrate your answer with an example of a p-block

More information

Directions: Multiple Choice For each of the following questions, choose the answer that best answers the question and place it on your answer sheet.

Directions: Multiple Choice For each of the following questions, choose the answer that best answers the question and place it on your answer sheet. CHEMISTRY TEST: THE PERIODIC TABLE Directions: Multiple Choice For each of the following questions, choose the answer that best answers the question and place it on your answer sheet. 1. Which of the following

More information

Review- The Periodic Table

Review- The Periodic Table Review- The Periodic Table Name Date Block Matching: Match the description in with the correct term in. Write the letter in the blank provided. Each term matches with only one description, so be sure to

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

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

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

Scientists create models to understand how things work, including atoms.

Scientists create models to understand how things work, including atoms. CHEM100 Week 4 Notes Page 1 of 6 Scientists create models to understand how things work, including atoms. Dalton created a theory for the atom with these 5 postulates 1. Elements consist of one or more

More information

Ion Formation Grade Nine

Ion Formation Grade Nine Ohio Standards Connection: Physical Sciences Benchmark A Describe that matter is made of minute particles called atoms and atoms are comprised of even smaller components. Explain the structure and properties

More information

2.5 The Modern View of Atomic Structure: An Introduction

2.5 The Modern View of Atomic Structure: An Introduction 2.5 The Modern View of Atomic Structure: An Introduction Figure 2.13 a & b (a) Expected Results of the Metal Foil Experiment if Thomson's Model Were Correct (b) Actual Results Copyright Houghton Mifflin

More information

Electrons In Atoms Mr. O Brien (SFHS) Chapter 5 Standard 1D

Electrons In Atoms Mr. O Brien (SFHS) Chapter 5 Standard 1D Electrons In Atoms Mr. O Brien (SFHS) Chapter 5 Standard 1D Electrons in Atoms (std.1d) What are Bohr Models? planetary model in which the negatively-charged electrons orbit a small, positively-charged

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

Atoms. Chemistry 100. Bettelheim, Brown, Campbell & Farrell. Introduction to General, Organic and Biochemistry Chapter 2

Atoms. Chemistry 100. Bettelheim, Brown, Campbell & Farrell. Introduction to General, Organic and Biochemistry Chapter 2 Chemistry 100 Bettelheim, Brown, Campbell & Farrell Ninth Edition Introduction to General, Organic and Biochemistry Chapter 2 Atoms Classifications of Matter: Elements An Element is a substance (for example,

More information

Worked solutions to student book questions Chapter 2 A particle view of matter

Worked solutions to student book questions Chapter 2 A particle view of matter Q1. Dalton and Thomson each proposed a model of an atom. a What experimental evidence did Thomson have that was not available to Dalton? b As a result of this experimental evidence, how did Thomson s model

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

Periodic Table Packet #1

Periodic Table Packet #1 Directions: Answer the questions with the proper information using your notes, book, and the periodic table. 1. Define a family. 2. What is a period? 3. What is the symbol for the following elements. a.

More information

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. Chem2A_Ch3_PT MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) The smallest amount of an element that retains that elementʹs characteristics is

More information

Name: Class: Date: ID: A

Name: Class: Date: ID: A Name: Class: Date: ID: A Chapter 5 Assessment Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Mendeleev arranged the elements in his periodic table in

More information

The Periodic Table of the Elements

The Periodic Table of the Elements Chapter 15 The Periodic Table of the Elements In Section 13.4, we saw the example of a square potential well. In that example, there were three bound states. This is the solution for a single electron

More information

3 Atomic Structure 15

3 Atomic Structure 15 3 Atomic Structure 15 3.1 Atoms You need to be familiar with the terms in italics The diameter of the nucleus is approximately 10-15 m and an atom 10-10 m. All matter consists of atoms. An atom can be

More information

Atoms and Ions (adapted from Chemistry A Guided Inquiry, Moog, R. S. and Farrell, J. J.)

Atoms and Ions (adapted from Chemistry A Guided Inquiry, Moog, R. S. and Farrell, J. J.) Atoms and Ions (adapted from Chemistry A Guided Inquiry, Moog, R. S. and Farrell, J. J.) There are 118 different elements currently on the periodic table. With the exception of technetium, all the elements

More information

02/27/14 Solution to the Assigned Problems of Workshop 2 Chem. 103, Spring 2014

02/27/14 Solution to the Assigned Problems of Workshop 2 Chem. 103, Spring 2014 Chapter 2: Atoms and the Periodic Table 02/27/14 Solution to the Assigned Problems of Workshop 2 Chem. 103, Spring 2014 Home-assigned problems (total of 15): 2.15, 2.17, 2.19, 2.21, 2.27, 2.29, 2.31, 2.37,

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

Bohr s Model of the Atom

Bohr s Model of the Atom Bohr Models Bohr s Model of the Atom Focuses on electrons and their arrangement. Bohr stated that electrons move with constant speed in fixed orbits around the nucleus, like planets around a sun. Bohr

More information

E α q 1 q 2 d. NOTE: The negative charge is the same distance from the positive charge in

E α q 1 q 2 d. NOTE: The negative charge is the same distance from the positive charge in During Class Invention Question: How are electrons arranged in an atom? 1. Describe the nature of the interaction between protons and electrons in an atom? Consider using some or all of the following terms

More information

Department of Physics and Geology The Elements and the Periodic Table

Department of Physics and Geology The Elements and the Periodic Table Department of Physics and Geology The Elements and the Periodic Table Physical Science 1422 Equipment Needed Qty Periodic Table 1 Part 1: Background In 1869 a Russian chemistry professor named Dmitri Mendeleev

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

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

electron configuration

electron configuration electron configuration Electron Configuration Knowing the arrangement of electrons in atoms will better help you understand chemical reactivity and predict an atom s reaction behavior. We know when n=1

More information

Chapter 3 Applying Your Knowledge- Even Numbered

Chapter 3 Applying Your Knowledge- Even Numbered Chapter 3 Applying Your Knowledge- Even Numbered 2. Elements in a specific compound are always present in a definite proportion by mass; for example, in methane, CH 4, 12 g of carbon are combined with

More information

Grade 9 Science Unit: Atoms and Elements Topic 4: Periodic Table & Compounds

Grade 9 Science Unit: Atoms and Elements Topic 4: Periodic Table & Compounds Grade 9 Science Unit: Atoms and Elements Topic 4: Periodic Table & Compounds Topic Using the Periodic Table Metals, Non- Metals & Metalloids I can Explain and identify the periods of the Periodic Table.

More information

Name Date Class ATOMIC STRUCTURE

Name Date Class ATOMIC STRUCTURE Name Date Class 4 ATOMIC STRUCTURE SECTION 4.1 DEFINING THE ATOM (pages 101 103) This section describes early atomic theories of matter and provides ways to understand the tiny size of individual atoms.

More information

Elements may combine in more than one proportion to form more than one compound. Examples...

Elements may combine in more than one proportion to form more than one compound. Examples... 1 UNIT 5 - ATOMIC THEORY: THE NUCLEAR MODEL OF THE ATOM 2 3 Dalton s Atomic Theory 1) Each element is made up of tiny, individual particles called atoms. 2) Atoms are indivisible; they cannot be created

More information

How Atoms Interact with Each Other

How Atoms Interact with Each Other Active Chemistry The Periodic Table Active Chemistry The Periodic Table Activity 8 ow Atoms Interact with Each Other GOALS In this activity you will: Relate patterns in ionization energies of elements

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

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

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

6. Each column of the periodic table is

6. Each column of the periodic table is 1. Atoms of elements that are in the same group have the same number of 5. Mendeleev left gaps in his periodic table because A. Protons B. Valence Electrons A. the table was too full B. no known elements

More information

EXPERIMENT 4: Electron Configuration of elements

EXPERIMENT 4: Electron Configuration of elements Material: laboratory display of the elements and a wall periodic table is required. Objective: To learn the use of periodic table for writing electron configuration of elements. INTRODUCTION Basic building

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

Theories of Matter Composition

Theories of Matter Composition Chapter 2 Theories of Matter Composition Democritus (5 th 4 th century BC) ATOMISM Aristotle (4 th 5 th century BC) CONTINUOUS MATTER FOUR ELEMENTS Earth, Air, Fire, Water Boyle (17 th century) Reintroduced

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

Mendeleev s Periodic Table of the Elements

Mendeleev s Periodic Table of the Elements Mendeleev s Periodic Table of the Elements Dmitri Mendeleev born 1834 in the Soviet Union. In 1869 he organised the 63 known elements into a periodic table based on atomic masses. He predicted the existence

More information

ELECTRON CONFIGURATION and BOHR-RUTHERFORD DIAGRAMS

ELECTRON CONFIGURATION and BOHR-RUTHERFORD DIAGRAMS ELECTRON CONFIGURATION and BOHR-RUTHERFORD DIAGRAMS I. Electron Arrangement. The electron configuration is a way of showing how the electrons are arranged in an atom. Recall that electrons are placed in

More information

ATOMS AND THE PERIODIC TABLE CHAPTER 3 PHYSICAL SCIENCE

ATOMS AND THE PERIODIC TABLE CHAPTER 3 PHYSICAL SCIENCE ATOMS AND THE PERIODIC TABLE CHAPTER 3 PHYSICAL SCIENCE Chapter 3 Vocabulary Words (27 words) Nucleus Atomic number Proton Mass number Neutron Isotopes Electron Atomic mass unit (amu) Energy level Average

More information

Mr. Dolgos Regents Chemistry NOTE PACKET. Unit 2: Atomic Theory

Mr. Dolgos Regents Chemistry NOTE PACKET. Unit 2: Atomic Theory *STUDENT* *STUDENT* Mr. Dolgos Regents Chemistry NOTE PACKET Unit 2: Atomic Theory 1 *STUDENT* UNIT 2 - ATOMIC THEORY *STUDENT* VOCABULARY: Allotrope Anion Atom Atomic Mass Atomic Mass unit (a.m.u.) Atomic

More information

Name: Period: Date: Unit 3 Practice Review (the questions on the test are NOT the same as the review questions)

Name: Period: Date: Unit 3 Practice Review (the questions on the test are NOT the same as the review questions) Name: Period: Date: Unit 3 Review: things you will need to know 1. Atomic Theories: Know all the scientists in order. What did they discover? What experiment did they use? 2. Development of the periodic

More information

Multiple Choice Identify the letter of the choice that best completes the statement or answers the question.

Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. Introduction to Chemistry Exam 2 Practice Problems 1 Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. 1.Atoms consist principally of what three

More information

Chapter -9. Classification of Elements The periodic Table

Chapter -9. Classification of Elements The periodic Table Chapter -9 Classification of Elements The periodic Table SYNOPSIS From the earliest times, scientists have been trying to classify the available elements on the basis of their properties. Dobereiner proposed

More information

Standardized Test Preparation. Chapter 3. Preview. Multiple Choice Short Answer Extended Response

Standardized Test Preparation. Chapter 3. Preview. Multiple Choice Short Answer Extended Response Preview Short Answer Extended Response 1. A chemical compound always has the same elements in the same proportions by mass regardless of the source of the compound. This is a statement of A. the law of

More information

Name Pre-Test : Atomic Structure and the Periodic Table

Name Pre-Test : Atomic Structure and the Periodic Table 1 Pre-Test : Atomic Structure and the Periodic Table Directions: Circle the letter to indicate whether the following statements are either true ( T ) or false ( F ). 1. Atomic structure refers to the building

More information

CHM1 Exam 4 Review. Topics. 1. Structure of the atom a. Proton nucleus + 1 amu b. Neutron nucleus 0 1 amu c. Electron orbits - 0 amu 2.

CHM1 Exam 4 Review. Topics. 1. Structure of the atom a. Proton nucleus + 1 amu b. Neutron nucleus 0 1 amu c. Electron orbits - 0 amu 2. Topics 1. Structure of the atom a. Proton nucleus + 1 amu b. Neutron nucleus 0 1 amu c. Electron orbits - 0 amu 2. Atomic symbols Mass number (protons + neutrons) 4+ charge 126C atomic number (# protons)

More information

Atomic Structure & the Periodic Table CHAPTERS 4 & 5

Atomic Structure & the Periodic Table CHAPTERS 4 & 5 Atomic Structure & the Periodic Table CHAPTERS 4 & 5 Objectives Understandings: Chemical structure determines the properties of matter The identity and properties of individual elements is determined by

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

Chapter NP-1. Nuclear Physics. Atomic Nature of Matter TABLE OF CONTENTS INTRODUCTION OBJECTIVES 1.0 PROPERTIES OF SUBSTANCES

Chapter NP-1. Nuclear Physics. Atomic Nature of Matter TABLE OF CONTENTS INTRODUCTION OBJECTIVES 1.0 PROPERTIES OF SUBSTANCES Chapter NP-1 Nuclear Physics Atomic Nature of Matter TABLE OF CONTENTS INTRODUCTION OBJECTIVES 1.0 PROPERTIES OF SUBSTANCES 1.1 CHEMICAL AND PHYSICAL PROPERTIES 2.0 COMPOSITION OF ATOMS 2.1 ATOMIC STRUCTURE

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

Atoms and the Periodic Table. Subatomic Particles

Atoms and the Periodic Table. Subatomic Particles Atoms and the Periodic Table Chapter Three Subatomic Particles Atoms are composed of subatomic particles Particle Symbol Mass (g) Mass (amu) Charge Proton p 1.672622 x 10-24 1.007276 +1 Neutron n 1.674927

More information