Chapter 8. Periodic Properties of the Element. Modified by Dr. Cheng-Yu Lai
|
|
|
- Hillary Burke
- 7 years ago
- Views:
Transcription
1 Chapter 8. Periodic Properties of the Element Modified by Dr. Cheng-Yu Lai
2 Energy Diagram for Hydrogen Atom The energy of a particular orbital is determined by its value of n. All orbitals with the same value of n have the same energy and are said to be degenerate. Hydrogen single electron occupy the lowest energy state, the ground state. If energy is put into the system, the electron can be transferred to higher energy orbital called excited state. For a one-electron hydrogen atom, orbitals on the same energy level have the same energy. That is, they are degenerate. H : 1s1 Orbital Energy Levels for the Hydrogen Atom
3 Electron Energy in Hydrogen-like Charge Atoms 2 Z 18 Eelectron x 10 J 2 n Z = nuclear charge (atomic number) n = energy level or principal quantum number (n) = 1, 2, 3, 4, ***Equation works only for atoms or ions with 1 electron (H, He+, Li2+, etc). Rydberg s constant (RH) = x J Johannes Rydberg ( )
4 Energy Orbitals for Polyelectronic Atoms As the number of electrons increases, though, so does the repulsion between them. Therefore, in manyelectron atoms, orbitals on the same energy level are no longer degenerate. For a given principal quantum level the orbitals vary in energy as follows: Ens< Enp < End < Enf
5 Order of Sublevel Filling in Ground State Electron Configurations Start by drawing a diagram, putting each energy shell on a row and listing the sublevels (s, p, d, f) for that shell in order of energy (from left to right). Next, draw arrows through the diagonals, looping back to the next diagonal each time Pearson Education, Inc. 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 6s 6p 6d 7s
6 Rules for Electron Configurations of Multielectron Atoms Electron Configuration: A description of which orbitals are occupied by electrons Degenerate Orbitals: Orbitals that have the same energy level. For example, the three p orbitals in a given subshell Ground-State Electron Configuration: The lowest-energy configuration Aufbau Principle ( building up ): A guide for determining the filling order of orbitals 2012 Pearson Education, Inc. Chapter 5/6
7 Ruls for Electron Configurations of Multielectron Atoms Rules of the aufbau principle: 1. Lower-energy orbitals fill before higher-energy orbitals. 2. An orbital can only hold two electrons, which must have opposite spins (Pauli exclusion principle). 3. If two or more degenerate orbitals are available, follow Hund s rule. Hund s Rule: If two or more orbitals with the same energy are available, one electron goes into each until all are halffull. The electrons in the half-filled orbitals all have the same value of their spin quantum number Pearson Education, Inc. Chapter 5/7
8 Electron Configurations of Multielectron Atoms Electron Configuration H: 1s1 1 electron s orbital (l = 0) n= Pearson Education, Inc. Chapter 5/8
9 Electron Configurations of Multielectron Atoms Electron Configuration H: 1s1 He: 1s2 2 electrons s orbital (l = 0) n= Pearson Education, Inc. Chapter 5/9
10 Electron Configurations of Multielectron Atoms Electron Configuration H: He: Li: 1s1 1s2 Lowest energy to highest energy 1s2 2s1 1 electron s orbital (l = 0) n= Pearson Education, Inc. Chapter 5/10
11 Electron Configurations of Multielectron Atoms Electron Configuration H: 1s1 He: 1s2 Li: 1s2 2s1 N: 1s2 2s2 2p3 3 electrons p orbital (l = 1) n= Pearson Education, Inc. Chapter 5/11
12 Orbital Diagrams As protons are added one by one to the nucleus to build up the elements, electrons are similarly added to these hydrogen-like orbitals. Each box represents one orbital. Half-arrows represent the electrons. The direction of the arrow represents the spin of the electron. H : 1s1, He : 1s2, Li : 1s2 2s1, Be : 1s2 2s2 B : 1s2 2s2 2p1, C : 1s2 2s2 2p2.
13 Electron Configurations of Multielectron Atoms Hund s Rule For degenerate orbitals, the lowest energy is attained when the number of electrons with the same spin is maximized. N : 1s2 2s2 2p3, O : 1s2 2s2 2p4, F : 1s2 2s2 2p5, Ne : 1s2 2s2 2p6, Na : 1s2 2s2 2p63s1 OR [Ne] 3s1
14 Electron Configurations of Multielectron Atoms Electron Configuration H: Orbital-Filling Diagram 1s1 1s He: 1s2 Li: 1s2 2s1 N: 1s2 2s2 2p Pearson Education, Inc. Chapter 5/14
15 Electron Configurations of Multielectron Atoms Electron Configuration H: Orbital-Filling Diagram 1s1 1s He: 1s2 1s Li: 1s2 2s1 N: 1s2 2s2 2p Pearson Education, Inc. Chapter 5/15
16 Electron Configurations of Multielectron Atoms Electron Configuration H: Orbital-Filling Diagram 1s1 1s He: 1s2 1s Li: 1s2 2s1 N: 1s2 2s2 2p3 1s 2s 2012 Pearson Education, Inc. Chapter 5/16
17 Electron Configurations of Multielectron Atoms Electron Configuration H: Orbital-Filling Diagram 1s1 1s He: 1s2 1s Li: 1s2 2s1 N: 1s2 2s2 2p3 1s 2s 1s 2s 2012 Pearson Education, Inc. 2p Chapter 5/17
18 Element Lithium Configuration notation Orbital notation 1s22s1 [He]2s1 1s Beryllium 2p [He]2s2 2s 2p 1s22s2p1 [He]2s2p1 1s Carbon 1s22s2p2 Nitrogen 1s22s2p3 Oxygen 1s22s2p4 Fluorine 1s22s2p5 2s 2p [He]2s2p2 1s 2s 2p [He]2s2p3 1s 2s 2p [He]2s2p4 1s 2s 2p [He]2s2p5 1s Neon 2s 1s22s2 1s Boron Noble gas notation 2s 2p 1s22s2p6 [He]2s2p6 1s 2s 2p
19 Electron Configurations of Multielectron Atoms Na: Electron Configuration Shorthand Configuration 1s2 2s2 2p6 3s1 [Ne] 3s1 Ne configuration P: 1s2 2s2 2p6 3s2 3p3 [Ne] 3s2 3p3 Ne configuration K: [Ar] 4s1 1s2 2s2 2p6 3s2 3p6 4s1 Ar configuration Sc: 1s2 2s2 2p6 3s2 3p6 4s2 3d1 Ar configuration [Ar] 4s2 3d1 Valence Shell: Outermost shell electrons.
20 Example 8.1 Electron Configurations Write electron configurations for each element. a. Mg b. P c. Br d. Al Solution a. Mg Magnesium has 12 electrons. Distribute 2 of these into the 1 s orbital, 2 into the 2s orbital, 6 into the 2p orbitals, and 2 into the 3s orbital. Mg 1s2 2s2 2p6 3s2 or [Ne] 3s2 b. P Phosphorus has 15 electrons. Distribute 2 of these into the 1s orbital, 2 into the 2s orbital, 6 into the 2p orbitals, 2 into the 3s orbital, and 3 into the 3p orbitals. P 1s2 2s2 2p6 3s2 3p3 or [Ne] 3s2 3p3 c. Br Bromine has 35 electrons. Distribute 2 of these into the 1s orbital, 2 into the 2s orbital, 6 into the 2p orbitals, 2 into the 3s orbital, 6 into the 3p orbitals, 2 into the 4s orbital, 10 into the 3d orbitals, and 5 into the 4p orbitals. Br 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5 or [Ar] 4s2 3d10 4p5 d. Al Aluminum has 13 electrons. Distribute 2 of these into the 1s orbital, 2 into the 2s orbital, 6 into the 2p orbitals, 2 into the 3s orbital, and 1 into the 3p orbital. Al 1s2 2s2 2p6 3s2 3p1 or [Ne] 3s2 3p1 Chemistry: A Molecular Approach, 3rd Edition Nivaldo J. Tro 2014 Pearson Education, Inc.
21 Example 8.2 Writing Orbital Diagrams Write the orbital diagram for sulfur and determine the number of unpaired electrons. Solution Since sulfur s atomic number is 16, it has 16 electrons and the electron configuration 1s2 2s2 2p6 3s2 3p4. Draw a box for each orbital, putting the lowest energy orbital (1s) on the far left and proceeding to orbitals of higher energy to the right. Distribute the 16 electrons into the boxes representing the orbitals, allowing a maximum of 2 electrons per orbital and remembering Hund s rule. You can see from the diagram that sulfur has two unpaired electrons. Two unpaired electrons Chemistry: A Molecular Approach, 3rd Edition Nivaldo J. Tro 2014 Pearson Education, Inc.
22 Valence Electrons The electrons in the outermost principle quantum level of an atom. Atom Valence Electrons Ca 2 N 5 Br 7 Valence electron is the most important electrons to us because they are involved in bonding. Elements with the same valence electron configuration show similar chemical behavior. Inner electrons are called core electrons.
23 Electron Configurations and the Periodic Table Valence Shell: Outermost shell electrons. Li: 2s1 Na: 3s1 Cl: 3s2 3p5 Br: 4s2 4p Pearson Education, Inc. Chapter 5/23
24 Electron Configurations and the Periodic Table
25 Example 8.3 Valence Electrons and Core Electrons Write the electron configuration for Ge. Identify the valence electrons and the core electrons. Solution Write the electron configuration for Ge by determining the total number of electrons from germanium s atomic number (32) and then distributing them into the appropriate orbitals. Ge 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p2 sodium 1s22s22p63s1 iron 1s22s22p63s23p64s23d6 bromine 1s22s22p63s23p64s23d104p5 barium Chemistry: A Molecular Approach, 3rd Edition Nivaldo J. Tro 1s22s22p63s23p64s23d104p65s24d105p66s Pearson Education, Inc.
26 Irregular Electron Configurations There are a few exceptions to the building-up order prediction for the ground state. Chromium (Z=24) and copper (Z=29) have been found by experiment to have the following ground-state electron configurations: Expected Cr = [Ar]4s23d4 Cu = [Ar]4s23d9 Found experimentally Cr = [Ar]4s13d5 Cu = [Ar]4s13d10 When it does this it becomes either a half fullshell (Cr) or a full one (Cu) this results in a more stable compound with lower energy. It only works if by removing and one electron from the s subshell an a half full or full subshell results Pearson Education, Inc.
27 H He Li Be B C N O F Ne Na Mg Al Si P S Cl Ar K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn 1s1 ELECTRONIC 1s2 CONFIGURATIONS 1s2 2s1 OF ELEMENTS s2 2s2 1s2 2s2 2p1 1s2 2s2 2p2 1s2 2s2 2p3 1s2 2s2 2p4 1s2 2s2 2p5 1s2 2s2 2p6 1s2 2s2 2p6 3s1 1s2 2s2 2p6 3s2 1s2 2s2 2p6 3s2 3p1 1s2 2s2 2p6 3s2 3p2 1s2 2s2 2p6 3s2 3p3 1s2 2s2 2p6 3s2 3p4 1s2 2s2 2p6 3s2 3p5 1s2 2s2 2p6 3s2 3p6 1s2 2s2 2p6 3s2 3p6 4s1 1s2 2s2 2p6 3s2 3p6 4s2 1s2 2s2 2p6 3s2 3p6 4s2 3d1 1s2 2s2 2p6 3s2 3p6 4s2 3d2 1s2 2s2 2p6 3s2 3p6 4s2 3d3 1s2 2s2 2p6 3s2 3p6 4s1 3d5 1s2 2s2 2p6 3s2 3p6 4s2 3d5 1s2 2s2 2p6 3s2 3p6 4s2 3d6 1s2 2s2 2p6 3s2 3p6 4s2 3d7 1s2 2s2 2p6 3s2 3p6 4s2 3d8 1s2 2s2 2p6 3s2 3p6 4s1 3d10 1s2 2s2 2p6 3s2 3p6 4s2 3d10
28 H He Li Be B C N O F Ne Na Mg Al Si P S Cl Ar K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn 1s1 ELECTRONIC 1s2 CONFIGURATIONS 1s2 2s1 OF ELEMENTS s2 2s2 1s2 2s2 2p1 1s2 2s2 2p2 1s2 2s2 2p3 1s2 2s2 2p4 1s2 2s2 2p5 1s2 2s2 2p6 1s2 2s2 2p6 3s1 1s2 2s2 2p6 3s2 1s2 2s2 2p6 3s2 3p1 1s2 2s2 2p6 3s2 3p2 1s2 2s2 2p6 3s2 3p3 1s2 2s2 2p6 3s2 3p4 1s2 2s2 2p6 3s2 3p5 1s2 2s2 2p6 3s2 3p6 1s2 2s2 2p6 3s2 3p6 4s1 1s2 2s2 2p6 3s2 3p6 4s2 1s2 2s2 2p6 3s2 3p6 4s2 3d1 1s2 2s2 2p6 3s2 3p6 4s2 3d2 1s2 2s2 2p6 3s2 3p6 4s2 3d3 1s2 2s2 2p6 3s2 3p6 4s1 3d5 1s2 2s2 2p6 3s2 3p6 4s2 3d5 1s2 2s2 2p6 3s2 3p6 4s2 3d6 1s2 2s2 2p6 3s2 3p6 4s2 3d7 1s2 2s2 2p6 3s2 3p6 4s2 3d8 1s2 2s2 2p6 3s2 3p6 4s1 3d10 1s2 2s2 2p6 3s2 3p6 4s2 3d10
29 Properties and Electron Configuration
30 Exam 5 11/20/13 Ch 8/9/10 45 Multiple choices only from ch8-10 review worksheet. Total points = 135 bank you scores Chem 101 Course Project 15 % Actual Grade ; returned by 12/02/13 3:00pm Password : DSUCHEM101 12/02 week 3 lectures for Course Project Review Please do show up attendance recommended/ required. 12/09/13 ACS exam Monday 3:30pm 5:30 pm- No Make up exam Need to inform chair 20% Actual Grade Chem 101 Student Online Course Evaluations Office hours: M 3:00-4:00 pm, T: 4:00-4:00 pm; W:3:00-4:00 pm Attendance and class participation Online HW Exams (5 exams) Course Project(11/04/13-12/02/13) ACS exam (comprehensive) 10%(5% from Lecture +5 % from Recitation) 13% 42% 15% 20% 100%
31 Element Lithium Configuration notation Orbital notation 1s22s1 [He]2s1 1s Beryllium 2p [He]2s2 2s 2p 1s22s2p1 [He]2s2p1 1s Carbon 1s22s2p2 Nitrogen 1s22s2p3 Oxygen 1s22s2p4 Fluorine 1s22s2p5 2s 2p [He]2s2p2 1s 2s 2p [He]2s2p3 1s 2s 2p [He]2s2p4 1s 2s 2p [He]2s2p5 1s Neon 2s 1s22s2 1s Boron Noble gas notation 2s 2p 1s22s2p6 [He]2s2p6 1s 2s 2p
32 ELECTRONIC CONFIGURATION OF IONS Positive ions (cations) are formed by removing electrons from atoms Negative ions (anions) are formed by adding electrons to atoms Electrons are removed first from the highest occupied orbitals (EXC. transition metals) SODIUM CHLORINE Na 1s2 2s2 2p6 3s1 Na+ 1s2 2s2 2p6 Cl 1s2 2s2 2p6 3s2 3p5 Cl 1s2 2s2 2p6 3s2 3p6 Group 1a atom: [Noble gas] ns1 1 electron removed from the 3s orbital 1 electron added to the 3p orbital -1 egroup 1a ion+: [Noble gas] Group 2a atom: [Noble gas] ns2-2 egroup 2a ion2+: [Noble gas]
33 Positive ions (cations) are formed by removing electrons from atoms Negative ions (anions) are formed by adding electrons to atoms Electrons are removed first from the highest occupied orbitals (EXC. transition metals) SODIUM CHLORINE Na 1s2 2s2 2p6 3s1 Na+ 1s2 2s2 2p6 Cl 1s2 2s2 2p6 3s2 3p5 Cl 1s2 2s2 2p6 3s2 3p6 1 electron removed from the 3s orbital 1 electron added to the 3p orbital Group 6a atom: [Noble gas] ns2 np4 +2 e- Group 6a ion2-: [Noble gas] ns2 np6 Group 7a atom: [Noble gas] ns2 np5 +1 e- Group 7a ion-: [Noble gas] ns2 np6 Chapter 6/ Pearson Education, Inc.
34 Electron Configurations of Ions Positive ions (cations) are formed by removing electrons from atoms Negative ions (anions) are formed by adding electrons to atoms Electrons are removed first from the highest occupied orbitals (EXC. transition metals) Atoms Ions Fe: [Ar] 4s2 3d6-2 e- Fe2+: [Ar] 3d6 Fe: [Ar] 4s2 3d6-3 e- Fe3+: [Ar] 3d5 FIRST ROW TRANSITION METALS Despite being of lower energy and being filled first, electrons in the 4s orbital are removed before any electrons in the 3d orbitals. TITANIUM Ti Ti+ Ti2+ Ti3+ Ti4+ 1s2 2s2 2p6 3s2 3p6 4s2 3d2 1s2 2s2 2p6 3s2 3p6 4s1 3d2 1s2 2s2 2p6 3s2 3p6 3d2 1s2 2s2 2p6 3s2 3p6 3d1 1s2 2s2 2p6 3s2 3p6
35 Electron Configurations of Transition Metal Cations in Their Ground State When transition metals form cations, the first electrons removed are the valence electrons, even though other electrons were added after. Electrons may also be removed from the sublevel closest to the valence shell after the valence electrons. The iron atom has two valence electrons: Fe atom = 1s22s22p63s23p64s23d6 When iron forms a cation, it first loses its valence electrons: Fe2+ cation = 1s22s22p63s23p63d6 It can then lose 3d electrons: Fe3+ cation = 1s22s22p63s23p63d Pearson Education, Inc.
36 Octet Rule Octet rule: Main-group elements tend to undergo reactions that leave them with eight outer-shell electrons. That is, main-group elements react so that they attain a noble-gas electron configuration with filled s and p sublevels in their valence electron shell. An octet means 8 valence electrons. is associated with the stability of the noble gases. Exception: Helium (He) is stable with 2 valence electrons. Electron level arrangement He 2 valence electrons 2 Ne 2, 8 8 Ar 2, 8, 8 8 Kr 2, 8, 18,
37 Metals Form Positive Ions Metals form positive ions by a loss of their valence electrons. with the electron configuration of the nearest noble gas. that have fewer electrons than protons. Group 1A metals ion 1+ Group 2A metals ion 2+ Group 3A metals ion 3+ Copyright 2005 by Pearson Education, Inc. Publishing as Benjamin Cummings 37
38 Formation of a Sodium Ion, Na+ Sodium achieves an octet by losing its one valence electron. 2, 8, 1 2, 8 38 Copyright 2005 by Pearson Education, Inc. Publishing as Benjamin Cummings
39 Learning Check - Aluminum A. The number of valence electrons in aluminum is 1) 1e-. 2) 2e-. 3) 3e-. B. The change in electrons for octet requires a 1) loss of 3e-. 2) gain of 3e-. 3) a gain of 5e-. C. The ionic charge of aluminum is 1) 3-. 2) 5-. 3) 3+. D. The symbol for the aluminum ion is 1) Al3+. 2) Al3-. 3) Al+. 39
40 Formation of Negative Ions In ionic compounds, nonmetals achieve an octet arrangement. gain electrons. form negatively charged ions with 3-, 2-, or 1charges. 40
41 Formation of a Chloride, ClChlorine achieves an octet by adding an electron to its valence electrons. 2, 8, 7 2, 8, 8 Copyright 2005 by Pearson Education, Inc. Publishing as Benjamin Cummings 41
42 Electron Configurations of Ions Matching Oxidation Number Chapter 6/ Pearson Education, Inc.
43
44 Example 8.6 Electron Configurations and Magnetic Properties for Ions Write the electron configuration and orbital diagram for each ion and determine whether each is diamagnetic or paramagnetic. a. Al3+ b. S2 c. Fe3+ Solution a. Al3+ Begin by writing the electron configuration of the neutral atom. Since this ion has a 3+ charge, remove three electrons to write the electron configuration of the ion. Write the orbital diagram by drawing half-arrows to represent each electron in boxes representing the orbitals. Because there are no unpaired electrons, Al3+ is diamagnetic. Al Al3+ [Ne] 3s2 3p1 [Ne] or [He] 2s2 2p6 Diamagnetic Continued b. S2 Write the orbital diagram by drawing half-arrows to represent each electron in boxes representing the orbitals. Because there are no unpaired electrons, S2 is diamagnetic. S S2 [Ne] 3s2 3p4 [Ne] 3s2 3p6 Chemistry: A Molecular Approach, 3rd Edition Nivaldo J. Tro Diamagnetic 2014 Pearson Education, Inc.
45 Example 8.6 Electron Configurations and Magnetic Properties for Ions Continued c. Fe3+ Begin by writing the electron configuration of the neutral atom. Since this ion has a 3+ charge, remove three electrons to write the electron configuration of the ion. Since it is a transition metal, remove the electrons from the 4s orbital before removing electrons from the 3d orbitals. Write the orbital diagram by drawing halfarrows to represent each electron in boxes representing the orbitals. There are unpaired electrons, so Fe3+ is paramagnetic. Fe Fe3+ [Ar] 4s2 3d6 [Ar] 4s0 3d5 Paramagnetic Chemistry: A Molecular Approach, 3rd Edition Nivaldo J. Tro 2014 Pearson Education, Inc.
46 Chapter 8. Periodic Properties of the Element Modified by Dr. Cheng-Yu Lai
47 1. Atomic Radius Definition: Half of the distance between nuclei in covalently bonded diatomic molecule Radius decreases across a period Increased effective nuclear charge due to decreased shielding Radius increases down a group Each row on the periodic table adds a shell or energy level to the atom
48 Table of Atomic Radii
49 Cation Formation Effective nuclear charge on remaining electrons increases. Na atom 1 valence electron 11p+ Valence elost in ion formation Result: a smaller sodium cation, Na+ Remaining e- are pulled in closer to the nucleus. Ionic size decreases.
50 Anion Formation Chlorine atom with 7 valence e17p+ One e- is added to the outer shell. Effective nuclear charge is reduced and the e- cloud expands. A chloride ion is produced. It is larger than the original atom.
51 Ionic Radii
52 Isoelectronic = same electron configuration
53 2. Ionization Energy Ionization Energy (Ei): The amount of energy necessary to remove the highest-energy electron from an isolated neutral atom in the gaseous state The energy required is called the first ionization energy. X(g) + energy X+ + e 2012 Pearson Education, Inc. Chapter 6/53
54 Ionization Energy The energy required to remove an electron from an atom is ionization energy. (measured in kilojoules, kj) The energy required is called the first ionization energy. X(g) + energy X+ + e- The larger the atom is, the easier its electrons are to remove. Ionization energy and atomic radius are inversely proportional. Ionization energy is always endothermic, that is energy is added to the atom to remove the electron. Chemistry: A Molecular Approach, 3rd Edition Nivaldo J. Tro 2014 Pearson Education, Inc.
55 Higher Ionization Energies M + energy M+ + e - M+ + energy M2+ + e- M2+ + energy M3+ + e- # OF VALENCE LECTRONS 2S1 2S2 2S3 2S4 2S5 2S6 2S7 2S8
56 Ionization Energy
57 Worked Example 6.2 Higher Ionization Energies Instructor Resource DVD for Chemistry, 6th Edition John McMurry & Robert C. Fay 2012 Pearson Education, Inc.
58 3. Electron Affinity - EA Energy is released when an neutral atom gains an electron. Gas state M(g) + 1e M1 (g) + EA Electron affinity is defined as exothermic ( ), The more energy that is released, the larger the electron affinity. The more negative the number, the larger the EA Pearson Education, Inc.
59 Electron Affinity Definition - the energy change associated with the addition of an electron Affinity tends to increase across a period Affinity tends to decrease as you go down in a period Electrons farther from the nucleus experience less nuclear attraction Some irregularities due to repulsive forces in the relatively small p orbitals
60 Electron Affinity Definition - the energy change associated with the addition of an electron
61 4. Metallic Character Metallic character is how closely an element s properties match the ideal properties of a metal. More malleable and ductile, better conductors, and easier to ionize Metallic character decreases left to right across a period. Metals found at the left of the period and nonmetals to the right Metallic character increases down the column. Nonmetals found at the top of the middle main group elements and metals found at the bottom 2014 Pearson Education, Inc.
62 Metallic Character in the Periodic Table
63 5. Electronegativity Electronegativity is a measure of an atom s attraction for another atom s electrons. It is an arbitrary scale that ranges from 0 to 4. The units of electronegativity are Paulings. Generally, metals are electron givers and have low electronegativities. Nonmetals are are electron takers and have high electronegativities.
64 The electron affinity is to attract any electron. The electronegativity is to attract the electrons in a covalent bond between that atom and another.
65 Summary of Trends
6.5 Periodic Variations in Element Properties
324 Chapter 6 Electronic Structure and Periodic Properties of Elements 6.5 Periodic Variations in Element Properties By the end of this section, you will be able to: Describe and explain the observed trends
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
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
Copyrighted by Gabriel Tang B.Ed., B.Sc.
Chapter 8: The Periodic Table 8.1: Development of the Periodic Table Johann Dobereiner: - first to discover a pattern of a group of elements like Cl, Br, and I (called triads). John Newland: - suggested
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
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
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.
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
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
Chapter Test. Teacher Notes and Answers 5 The Periodic Law TEST A 1. b 2. d 3. b 4. b 5. d 6. a 7. b 8. b 9. b 10. a 11. c 12. a.
Assessment Chapter Test A Teacher Notes and Answers 5 The Periodic Law TEST A 1. b 2. d 3. b 4. b 5. d 6. a 7. b 8. b 9. b 10. a 11. c 12. a 13. c 14. d 15. c 16. b 17. d 18. a 19. d 20. c 21. d 22. a
Student Exploration: Electron Configuration
Name: Date: Student Exploration: Electron Configuration Vocabulary: atomic number, atomic radius, Aufbau principle, chemical family, diagonal rule, electron configuration, Hund s rule, orbital, Pauli exclusion
Unit 2 Periodic Behavior and Ionic Bonding
Unit 2 Periodic Behavior and Ionic Bonding 6.1 Organizing the Elements I. The Periodic Law A. The physical and chemical properties of the elements are periodic functions of their atomic numbers B. Elements
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
Section 11.3 Atomic Orbitals Objectives
Objectives 1. To learn about the shapes of the s, p and d orbitals 2. To review the energy levels and orbitals of the wave mechanical model of the atom 3. To learn about electron spin A. Electron Location
Molecular Models & Lewis Dot Structures
Molecular Models & Lewis Dot Structures Objectives: 1. Draw Lewis structures for atoms, ions and simple molecules. 2. Use Lewis structures as a guide to construct three-dimensional models of small molecules.
The Periodic Table; Chapter 5: Section 1 - History of the Periodic Table Objectives: Explain the roles of Mendeleev and Moseley in the development of
The Periodic Table; Chapter 5: Section 1 - History of the Periodic Table Objectives: Explain the roles of Mendeleev and Moseley in the development of the periodic table. Describe the modern periodic table.
IONISATION ENERGY CONTENTS
IONISATION ENERGY IONISATION ENERGY CONTENTS What is Ionisation Energy? Definition of t Ionisation Energy What affects Ionisation Energy? General variation across periods Variation down groups Variation
The Advanced Placement Examination in Chemistry. Part I Multiple Choice Questions Part II Free Response Questions Selected Questions from1970 to 2010
The Advanced Placement Examination in Chemistry Part I Multiple Choice Questions Part II Free Response Questions Selected Questions from1970 to 2010 Atomic Theory and Periodicity Part I 1984 1. Which of
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
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
Chapter 8 Atomic Electronic Configurations and Periodicity
Chapter 8 Electron Configurations Page 1 Chapter 8 Atomic Electronic Configurations and Periodicity 8-1. Substances that are weakly attracted to a magnetic field but lose their magnetism when removed from
REVIEW QUESTIONS Chapter 8
Chemistry 101 ANSWER KEY REVIEW QUESTIONS Chapter 8 Use only a periodic table to answer the following questions. 1. Write complete electron configuration for each of the following elements: a) Aluminum
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
IONISATION ENERGY CONTENTS
IONISATION ENERGY IONISATION ENERGY CONTENTS What is Ionisation Energy? Definition of t Ionisation Energy What affects Ionisation Energy? General variation across periods Variation down groups Variation
Chapter 7. Electron Structure of the Atom. Chapter 7 Topics
Chapter 7 Electron Structure of the Atom Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 1 Chapter 7 Topics 1. Electromagnetic radiation 2. The Bohr model of
ELECTRON CONFIGURATION (SHORT FORM) # of electrons in the subshell. valence electrons Valence electrons have the largest value for "n"!
179 ELECTRON CONFIGURATION (SHORT FORM) - We can represent the electron configuration without drawing a diagram or writing down pages of quantum numbers every time. We write the "electron configuration".
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
Chapter 3, Elements, Atoms, Ions, and the Periodic Table
1. Which two scientists in 1869 arranged the elements in order of increasing atomic masses to form a precursor of the modern periodic table of elements? Ans. Mendeleev and Meyer 2. Who stated that the
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
KEY. Honors Chemistry Assignment Sheet- Unit 3
KEY Honors Chemistry Assignment Sheet- Unit 3 Extra Learning Objectives (beyond regular chem.): 1. Related to electron configurations: a. Be able to write orbital notations for s, p, & d block elements.
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
Chapter 3. Elements, Atoms, Ions, and the Periodic Table
Chapter 3. Elements, Atoms, Ions, and the Periodic Table The Periodic Law and the Periodic Table In the early 1800's many elements had been discovered and found to have different properties. In 1817 Döbreiner's
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
Ch. 9 - Electron Organization. The Bohr Model [9.4] Orbitals [9.5, 9.6] Counting Electrons, configurations [9.7]
![Ch. 9 - Electron Organization. The Bohr Model [9.4] Orbitals [9.5, 9.6] Counting Electrons, configurations [9.7]](/thumbs/27/11797291.jpg "Ch. 9 - Electron Organization. The Bohr Model [9.4] Orbitals [9.5, 9.6] Counting Electrons, configurations [9.7]")
Ch. 9 - Electron Organization The Bohr Model [9.4] Orbitals [9.5, 9.6] Counting Electrons, configurations [9.7] Predicting ion charges from electron configurations. CHEM 100 F07 1 Organization of Electrons
Bonds. Bond Length. Forces that hold groups of atoms together and make them function as a unit. Bond Energy. Chapter 8. Bonding: General Concepts
Bonds hapter 8 Bonding: General oncepts Forces that hold groups of atoms together and make them function as a unit. Bond Energy Bond Length It is the energy required to break a bond. The distance where
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
MODERN ATOMIC THEORY AND THE PERIODIC TABLE
CHAPTER 10 MODERN ATOMIC THEORY AND THE PERIODIC TABLE SOLUTIONS TO REVIEW QUESTIONS 1. Wavelength is defined as the distance between consecutive peaks in a wave. It is generally symbolized by the Greek
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
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
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
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
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.
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
Unit 3.2: The Periodic Table and Periodic Trends Notes
Unit 3.2: The Periodic Table and Periodic Trends Notes The Organization of the Periodic Table Dmitri Mendeleev was the first to organize the elements by their periodic properties. In 1871 he arranged the
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
Chemistry: The Periodic Table and Periodicity
Chemistry: The Periodic Table and Periodicity Name: per: Date:. 1. By what property did Mendeleev arrange the elements? 2. By what property did Moseley suggest that the periodic table be arranged? 3. What
Chapter 5 Periodic Table. Dmitri Mendeleev: Russian Chemist credited with the discovery of the periodic table.
Chapter 5 Periodic Table Dmitri Mendeleev: Russian Chemist credited with the discovery of the periodic table. How did he organize the elements? According to similarities in their chemical and physical
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.
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
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)
Find a pair of elements in the periodic table with atomic numbers less than 20 that are an exception to the original periodic law.
Example Exercise 6.1 Periodic Law Find the two elements in the fifth row of the periodic table that violate the original periodic law proposed by Mendeleev. Mendeleev proposed that elements be arranged
Horizontal Rows are called Periods. Elements in the same period have the same number of energy levels for ground state electron configurations.
The Periodic Table Horizontal Rows are called Periods. Elements in the same period have the same number of energy levels for ground state electron configurations. Vertical Rows are called Families or Groups.
Be (g) Be + (g) + e - O (g) O + (g) + e -
2.13 Ionisation Energies Definition :First ionisation energy The first ionisation energy is the energy required when one mole of gaseous atoms forms one mole of gaseous ions with a single positive charge
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
Chapter 7. Chemistry, The Central Science, 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten
Chemistry, The Central Science, 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Chapter 7 John D. Bookstaver St. Charles Community College Cottleville, MO Development of 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
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
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
MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
Practice Questions - Chapter 7 Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Which one of the following represents an impossible set of
Chapter 8 Concepts of Chemical Bonding
Chapter 8 Concepts of Chemical Bonding Chemical Bonds Three types: Ionic Electrostatic attraction between ions Covalent Sharing of electrons Metallic Metal atoms bonded to several other atoms Ionic Bonding
CHAPTER 9 ATOMIC STRUCTURE AND THE PERIODIC LAW
CHAPTER 9 ATOMIC STRUCTURE AND THE PERIODIC LAW Quantum mechanics can account for the periodic structure of the elements, by any measure a major conceptual accomplishment for any theory. Although accurate
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
Periodic Trends for Electronegativity... 1. Periodic Trends for Ionization Energy... 3. Periodic Trends for Electron Affinity... 5
Periodic Trends Periodic trends are certain patterns that describe specific aspects of the elements in the periodic table, such as size and properties with electrons. The main periodic trends include:
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
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:
Questions on Chapter 8 Basic Concepts of Chemical Bonding
Questions on Chapter 8 Basic Concepts of Chemical Bonding Circle the Correct Answer: 1) Which ion below has a noble gas electron configuration? A) Li 2+ B) Be 2+ C) B2+ D) C2+ E) N 2-2) Of the ions below,
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
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
A pure covalent bond is an equal sharing of shared electron pair(s) in a bond. A polar covalent bond is an unequal sharing.
CHAPTER EIGHT BNDING: GENERAL CNCEPT or Review 1. Electronegativity is the ability of an atom in a molecule to attract electrons to itself. Electronegativity is a bonding term. Electron affinity is the
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
AP Chemistry A. Allan Chapter 8 Notes - Bonding: General Concepts
AP Chemistry A. Allan Chapter 8 Notes - Bonding: General Concepts 8.1 Types of Chemical Bonds A. Ionic Bonding 1. Electrons are transferred 2. Metals react with nonmetals 3. Ions paired have lower energy
Question: Do all electrons in the same level have the same energy?
Question: Do all electrons in the same level have the same energy? From the Shells Activity, one important conclusion we reached based on the first ionization energy experimental data is that electrons
CHAPTER 8 PRACTICE TEST QUESTIONS (END OF CHAPTER 7 TOO)
CHAPTER 8 PRACTICE TEST QUESTIONS (END OF CHAPTER 7 TOO) Information that most likely will be on the front cover of your exam: h i Z 2 ΔE = @ 2.18 x 10 @ 18 f Z 2 f J j @ k n f 2 n i 2 1. Which of the
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
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
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
Chemistry - Elements Electron Configurations The Periodic Table. Ron Robertson
Chemistry - Elements Electron Configurations The Periodic Table Ron Robertson History of Chemistry Before 16 th Century Alchemy Attempts (scientific or otherwise) to change cheap metals into gold no real
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
Unit 3: Quantum Theory, Periodicity and Chemical Bonding
Selected Honour Chemistry Assignment Answers pg. 9 Unit 3: Quantum Theory, Periodicity and Chemical Bonding Chapter 7: The Electronic Structure of Atoms (pg. 240 to 241) 48. The shape of an s-orbital is
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
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,
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.
CHAPTER 8 THE PERIODIC TABLE
CHAPTER 8 THE PERIODIC TABLE 8.1 Mendeleev s periodic table was a great improvement over previous efforts for two reasons. First, it grouped the elements together more accurately, according to their properties.
Electron Arrangements
Section 3.4 Electron Arrangements Objectives Express the arrangement of electrons in atoms using electron configurations and Lewis valence electron dot structures New Vocabulary Heisenberg uncertainty
CHAPTER 8 ELECTRON CONFIGURATION AND CHEMICAL PERIODICITY
CHAPTER 8 ELECTRON CONFIGURATION AND CHEMICAL PERIODICITY 8.1 Elements are listed in the periodic table in an ordered, systematic way that correlates with a periodicity of their chemical and physical properties.
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
Test Review Periodic Trends and The Mole
Test Review Periodic Trends and The Mole The Mole SHOW ALL WORK ON YOUR OWN PAPER FOR CREDIT!! 1 2 (NH42SO2 %N 24.1 %H 6.9 %S 27.6 %O 41.3 % Al %C 35.3 %H 4.4 %O 47.1 Al(C2H3O23 13.2 3 How many moles are
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
THE PERIODIC TABLE O F T H E E L E M E N T S. The Academic Support Center @ Daytona State College (Science 117, Page 1 of 27)
THE PERIODIC TABLE O F T H E E L E M E N T S The Academic Support Center @ Daytona State College (Science 117, Page 1 of 27) THE PERIODIC TABLE In 1872, Dmitri Mendeleev created the periodic table arranged
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
Atoms and Elements. Outline Atoms Orbitals and Energy Levels Periodic Properties Homework
Atoms and the Periodic Table The very hot early universe was a plasma with cationic nuclei separated from negatively charged electrons. Plasmas exist today where the energy of the particles is very high,
Periodic Table. 1. In the modern Periodic Table, the elements are arranged in order of increasing. A. atomic number B. mass number
Name: ate: 1. In the modern, the elements are arranged in order of increasing. atomic number. mass number. oxidation number. valence number 5. s the elements in Group I are considered in order of increasing
3) Of the following, radiation has the shortest wavelength. A) X-ray B) radio C) microwave D) ultraviolet E) infrared Answer: A
1) Which one of the following is correct? A) ν + λ = c B) ν λ = c C) ν = cλ D) λ = c ν E) νλ = c Answer: E 2) The wavelength of light emitted from a traffic light having a frequency of 5.75 1014 Hz is.
Chem 1A Exam 2 Review Problems
Chem 1A Exam 2 Review Problems 1. At 0.967 atm, the height of mercury in a barometer is 0.735 m. If the mercury were replaced with water, what height of water (in meters) would be supported at this pressure?
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
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
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
It takes four quantum numbers to describe an electron. Additionally, every electron has a unique set of quantum numbers.
So, quantum mechanics does not define the path that the electron follows; rather, quantum mechanics works by determining the energy of the electron. Once the energy of an electron is known, the probability
Electron Configuration Worksheet (and Lots More!!)
Electron Configuration Worksheet (and Lots More!!) Brief Instructions An electron configuration is a method of indicating the arrangement of electrons about a nucleus. A typical electron configuration
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