chapter-3-Atomic-Structure-and-the-Periodic-Table-1-1.ppt

Chapter 3
Table of Contents
Copyright © Cengage Learning. All rights reserved 1
3.1 Internal Structure of an Atom
3.2 Atomic Number and Mass Number
3.3 Isotopes and Atomic Masses
3.4 The Periodic Law and the Periodic Table
3.5 Metals and Nonmetals
3.6 Electron Arrangements Within Atoms
3.7 Electron Configurations and Orbital Diagrams
3.8 The Electronic Basis for the Periodic Law and the
Periodic Table
3.9 Classification of the Elements
Atomic Structure and the Periodic Table

Internal Structure of an Atom
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Section 3.1
• A very small particle that is a building block for
atoms.
Subatomic Particle

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Section 3.1
• The atom contains:
 Electrons – found outside the nucleus;
possesses a negative electrical charge;
smallest mass.
 Protons – found in the nucleus; positive
charge equal in magnitude to the electron’s
negative charge.
 Neutrons – found in the nucleus; no charge;
virtually same mass as a proton.
Three Types of Subatomic Particles

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Section 3.1
Charge and Mass Characteristics

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Section 3.1
• The nucleus is:
– Small compared with the overall size of the
atom.
– Extremely dense; accounts for almost all of
the atom’s mass.
– Positively charged center of an atom.

Return to TOC
Section 3.1
• An atom as a whole is electrically neutral (no net
electrical charge).
# of Protons = # of Electrons
Charge Neutrality of an Atom

Section 3.2
Atomic Number and Mass Number
• Atomic Number (Z) – # of protons in the nucleus
of an atom.
• Mass Number (A) – sum of the # of protons and
the # of neutrons in the nucleus of an atom.

Section 3.2
Complete Chemical Symbol Notation
23
11
Na
Mass number
Symbol
A
Z
Atomic number
Chemical symbol

Section 3.2
• A pure substance in which all atoms present
have the same atomic number.
• All atoms with the same atomic number have the
same chemical properties and are atoms of the
same element.
Element

Section 3.3
Isotopes and Atomic Masses
• Atoms of an element that have the same
number of protons and the same number of
electrons but different numbers of neutrons.
• Show almost identical chemical properties;
chemistry of atom is due to its electrons.
• Physical properties are often slightly different
because they have different masses.
• In nature most elements contain mixtures of
isotopes.
Isotopes

Section 3.3
Two Isotopes of Sodium
• Number of Protons = 11
• Mass number = 23
• Number of Neutrons = 12
• Number of Protons = 11
• Mass number = 24
• Number of Neutrons = 13
23
11
Na 24
11
Na

Section 3.3
Exercise
A certain isotope X contains 23 protons and 28
neutrons.
• What is the mass number of this isotope?
• Identify the element.

Section 3.3
Exercise
A certain isotope X contains 23 protons and 28
neutrons.
• What is the mass number of this isotope?
51
• Identify the element.
Vanadium

Section 3.3
• Elements occur in nature as mixtures of
isotopes.
• Carbon = 98.89% 12C
1.11% 13C
<0.01% 14C
• Calculated average mass for the isotopes of an
element expressed on a scale where
serves as the reference point.
Atomic Masses
12
6
C

Section 3.3
98.89% of 12 amu + 1.11% of 13.0034 amu =
Average Atomic Mass for Carbon
(0.9889)(12 amu) + (0.0111)(13.0034 amu) =
12.01 amu

Section 3.3
Exercise
An element consists of 62.60% of an isotope
with mass 186.956 amu and 37.40% of an
isotope with mass 184.953 amu.
• Calculate the average atomic mass and
identify the element.
Average Atomic Mass = 186.207 amu
The element is rhenium (Re).

Section 3.4
The Periodic Law and the Periodic Table
• Periodic Law – When elements are arranged in
order of increasing atomic number, elements
with similar chemical properties occur at periodic
(regularly recurring) intervals.
• Periodic Table – Tabular arrangement of the
elements in order of increasing atomic number
such that elements having similar chemical
properties are positioned in vertical columns.

Section 3.4
• Periods – horizontal rows of elements
• Groups – elements in the same vertical
columns; have similar chemical properties
The Periodic Table

Section 3.4
The Periodic Table

Section 3.4
• Table of common charges formed when creating
ionic compounds.
Groups
Group Charge
Alkali Metals (1A) 1+
Alkaline Earth Metals (2A) 2+
Halogens (7A) 1-
Noble Gases (8A) 0

Section 3.5
Metals and Nonmetals
• An element that has the
characteristic properties
of luster, thermal
conductivity, electrical
conductivity, and
malleability.
Metal

Section 3.5
• An element
characterized by the
absence of the
properties of luster,
thermal conductivity,
electrical conductivity,
and malleability.
Nonmetal

Section 3.5
Selected Physical Properties of Metals and Nonmetals

Section 3.5
Dividing Line Between Metals and Nonmetals

Section 3.6
Electron Arrangements Within Atoms
Electron Shells
• A region of space about a nucleus that contains
electrons that have approximately the same
energy and that spend most of their time
approximately the same distance from the
nucleus.
• Electrons that occupy the first electron shell are
closer to the nucleus and have a lower energy
than electrons in the second electron shell.

Section 3.6
Electron Subshells
• A region of space within an electron shell that
contains electrons that have the same energy.
Subshell Number of Electrons
s 2
p 6
d 10
f 14

Section 3.6
Electron Orbitals
• A region of space within an electron subshell
where an electron with a specific energy is most
likely to be found.
• An electron orbital can accommodate a
maximum of 2 electrons.

Section 3.6
Electron Orbitals
Subshell Number of Orbitals
s 1
p 3
d 5
f 7

Section 3.6
Electron Orbitals

Section 3.6
Orbitals Within the Same Subshell Differ in Orientation

Section 3.6
Electron Spin
• As an electron “moves about” within an orbital,
it spins on its own axis in either a clockwise or a
counterclockwise direction.
• When two electrons are present in an orbital,
they always have opposite spins.

Section 3.7
Electron Configurations and Orbital Diagrams
Rules for Assigning Electrons to Various Shells, Subshells, and
Orbitals
1. Electron subshells are filled in order of
increasing energy.
2. Electrons occupy the orbitals of a subshell such
that each orbital acquires one electron before
any orbital acquires a second electron. All
electrons in such singly occupied orbitals must
have the same spin.
3. No more than two electrons may exist in a
given orbital – and then only if they have
opposite spins.

Section 3.7
Subshell Energy Order

Section 3.7
Electron Configurations
• A statement of how many electrons an atom has
in each of its electron subshells.
• An oxygen atom as an electron arrangement of
two electrons in the 1s subshell, two electrons in
the 2s subshell, and four electrons in the 2p
subshell.
Oxygen: 1s22s22p4

Section 3.7
Electron Configurations

Section 3.7
Orbital Diagrams
• A notation that shows how many electrons an
atom has in each of its occupied electron
orbitals.
Oxygen: 1s22s22p4
Oxygen: 1s 2s 2p

Section 3.7
Exercise
Determine the expected electron
configurations for each of the following.
a) S
b) Ba

Section 3.7
Exercise
Determine the expected electron
configurations for each of the following.
a) S
1s22s22p63s23p4
b) Ba
1s22s22p63s23p64s23d104p65s24d105p66s2

Section 3.8
The Electronic Basis for the Periodic Law and the Periodic Table
• The electron arrangement in the outermost shell
is the same for elements in the same group.
• This is why elements in the same group have
similar chemical properties.
 Group 1A – very reactive
Li: 1s22s1
Na: 1s22s22p63s1
K: 1s22s22p63s23p64s1

Section 3.8
Electron Configurations and the Periodic Table

Section 3.8
Distinguishing Electron
• Last electron added to the electron configuration
for an element when electron subshells are filled
in order of increasing energy.
• This last electron is the one that causes an
element’s electron configuration to differ from
that of an element immediately preceding it in
the periodic table.

Section 3.9
Classification of the Elements
1. A system based on selected physical properties
of the elements, in which they are described as
metals or nonmetals.
2. A system based on the electron configurations
of the elements, in which elements are
described as noble-gas, representative,
transition, or inner transition elements.

Section 3.9
Classification of the Elements
Classification Scheme on the Periodic Table

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