1. Atomic Number, Mass Number, and Isotopes
2.3
All atoms can be identified by the number of protons and neutrons they contain.
The atomic number (Z) is the number of protons in the nucleus.
Protons determine the identity of an element. For example, nitrogen’s atomic number is 7, so every nitrogen has 7 protons.
The mass number (A) is the total number of protons and neutrons.
Protons and neutrons are collectively referred to as nucleons.
Mass number
(number of protons + neutrons)
Elemental symbol
Atomic number
(number of protons)

2. Atomic Number, Mass Number, and Isotopes
Most elements have two or more isotopes, atoms that have the same atomic number (Z) but different mass numbers (A).
1 proton
0 neutrons
1 proton
1 neutron
1 proton
2 neutrons
Isotopes of the same element exhibit similar chemical properties, forming the same types of compounds and displaying similar reactivities.

3. 2.4
Nuclear Stability
The number of protons and neutrons present in an atom determine the stability of the nucleus – will discuss in detail in chapter 20 (CHMY 172)

4. 1 amu = 1/12 the mass of a carbon-12 atom
2.5
Average Atomic Mass
Atomic mass is the mass of an atom in atomic mass units (amu).
1 amu = 1/12 the mass of a carbon-12 atom
The average atomic mass on the periodic table represents the average mass of the naturally occurring mixture of isotopes.
Average mass (C) = (0.9893)( amu) + (0.0107)( amu)
Which isotope has a greater abundance naturally, bromine-79 or bromine-81?
Isotope
Isotopic mass (amu)
Natural abundance (%)
12C
98.93
13C
1.07
= amu

5. Average Atomic Mass
Measuring Atomic Mass
The most direct and most accurate method for determining atomic and molecular masses is mass spectrometry, using a mass spectrometer.
The mass spectrum of neon

6. Worked Example 2.1
Determine the numbers of protons, neutrons, and electrons in each of the following species: (a) Cl, (b) Cl, (c) K, and (d) carbon-14. 35 17 37 41
Strategy Recall the superscript denotes the mass number (A) and the subscript denotes the atomic number (Z). If no subscript is shown, the atomic number can be deduced from the elemental symbol or name. There is no charge shown on these atoms.
Text Practice: a)

7. 2.6
The Periodic Table
The periodic table is a chart in which elements having similar chemical and physical properties are grouped together.

8. The Periodic Table
Elements are arranged in periods, horizontal rows, in order of increasing atomic number.

9. The Periodic Table
Elements can be categorized as metals, nonmetals, or metalloids.
Metals are good conductors
of heat and electricity.
Nonmetals are poor
conductors of heat or
electricity.
Metalloids have
intermediate properties.

10. The Periodic Table
A vertical column is known as a group.

11. The Periodic Table
Group 1A elements (Li, Na, K, Rb, Cs, Fr) are called alkali metals.

12. The Periodic Table
Group 2A elements (Be, Mg, Ca, Sr, Ba, Ra) are called alkaline earth metals.

13. The Periodic Table
Group 6A elements (O, S, Se, Te, Po) are called chalcogens.

14. The Periodic Table
Group 7A elements (F, Cl, Br, I, At) are called halogens.

15. The Periodic Table
Group 8A elements (He, Ne, Ar, Kr, Xe, Rn) are called the noble gases.

16. The Periodic Table
Groups 1B and 3B-8B are called the transition elements or transition metals.

17. Chemistry: Atoms First Second Edition Julia Burdge & Jason Overby
Chapter 3
Quantum Theory and the Electronic Structure of Atoms
M. Stacey Thomson
Pasco-Hernando State College
Copyright (c) The McGraw-Hill Companies, Inc. Permission required for reproduction or display.

18. Energy and Energy Changes
3.1
Energy is the capacity to do work or transfer heat.
Energy is either kinetic or potential.
Kinetic energy (Ek) is the energy of motion.
m is the mass of the object
u is its velocity
One form of kinetic energy of particular interest to chemists is thermal energy, which is the energy associated with the random motion of atoms and molecules.

19. Forms of Energy
Potential energy is the energy possessed by an object by virtue of its position or stability.
There are two forms of potential energy of great interest to chemists:
Chemical energy is energy stored within the structural units of chemical substances.
Electrostatic energy is potential energy that results from the interaction of charged particles.
Q1 and Q2 represent two charges separated by the distance, d.

20. Energy and Energy Changes
Kinetic and potential energy are interconvertible – one can be converted to the other.
Although energy can assume many forms, the total energy of the universe is constant.
Energy can neither be created nor destroyed.
When energy of one form disappears, the same amount of energy reappears in another form or forms.
This is known as the law of conservation of energy.
(activities 2-7)
Text Practice: 3.4

21. Units of Energy
The SI unit of energy is the joule (J), named for the English physicist James Joule.
It is the amount of energy possessed by a 2-kg mass moving at a speed of 1 m/s.
Ek = ½ mu2 = ½(2 kg)(1 m/s)2 = 1 kg∙m2/s2 = 1 J
The joule can also be defined as the amount of energy exerted when a force of 1 newton (N) is applied over a distance of 1 meter.
1 J = 1 N · m
Because the magnitude of a joule is so small, we often express large amounts of energy using the unit kilojoule (kJ).
1 kJ = 1000 J

22. Study Guide for sections 2.3-2.6, 3.1
DAY 4, Terms to know:
Sections , 3.1 atomic number, mass number, isotope, average mass, isotopic natural abundance, periodic table, halogens, noble gasses, transition metals, energy, kinetic energy, thermal energy, potential energy, chemical energy, electrostatic energy, law of conservation of energy, joule
DAY 4, Specific outcomes and skills that may be tested on exam 1:
Sections , 3.1
Be able to use elemental symbols to determine how many protons, neutrons, and electrons are present in an atom
Given a specific number of protons, neutrons, and electrons, be able to give a complete elemental symbol including element, mass, and charge
Given isotopes and their natural abundance, be able to calculate the average atomic mass
Given an average atomic mass and two or three isotopes, be able to describe the isotopes relative abundances
Be able to describe possible transformations from one form of energy to another
Given a process that involve a transfer of energy, be able to describe to describe what forms of energy exist before and after the process

23. Extra Practice Problems for sections 2.3-2.6, 3.1
Complete these problems outside of class until you are confident you have learned the SKILLS in this section outlined on the study guide and we will review some of them next class period

24. Prep for day 5 Must watch videos: Other helpful videos:
the lesson videos, but you don't have to watch the other videos such as the quiz videos and demos, although hey are also helpful (UC-Berkeley watch lessons 3-6 in module 2: light and matter, particles and waves). Also, you may skip sections of the videos that focus on solving the equations quantitatively.  We will be focusing on the conceptual analysis rather than the plug and chug.
Other helpful videos:
(MIT lectures 4 and 5)
(UC-Irvine lectures 3-5)
Read sections: