Ch. 7 Electron Configuration and Periodic Table

Question 1

Based on the type of subshell containing the outermost electrons, elements can be divided into ____?

Answer 1

Categories

Question 2

What are the 6 categories that elements are divided into on the periodic table?

Answer 2

1. Main Group Elements
2. Noble Gases
3. Transition Metals
4. Volatile Metals
5. Lanthanides
6. Actinides

Question 3

What part of the periodic table makes up the main group elements?

Answer 3

Groups 1A-7A

Question 4

What part of the periodic table makes up Noble Gases?

Answer 4

Group 8A

Question 5

What part of the periodic table makes up Transition Elements?

Answer 5

Group 3-11

Question 6

What part of the periodic table makes up Volatile Metals?

Answer 6

Group 12

Question 7

What part of the periodic table makes up the Lanthanides and Actinides?

Answer 7

Floating grid

Question 8

The key to periodicity is____.

Answer 8

Atomic Number

Question 9

Elements in a column of the modern periodic table have very similar ____ properties.

Answer 9

Chemical

Question 10

An outer electron feels an ____ to the nucleus and a ____ to an inner electron. This is known as What?

Answer 10

Attraction
Repulsion
Shielding or Screening

Question 11

Core electrons are most effective at shielding ___ ___.

Answer 11

Valence Electrons

Question 12

The number of protons and the number of valence electrons increase from ___ to ____. Therefore so does the Zeff.

Answer 12

Left to right

Across a period

Question 13

This is the magnitude of positive charge that is “felt” by a shielded electron. It is always positive.

Answer 13

Effective Nuclear Charge, Zeff

Question 14

Because of shielding the effective nuclear charge is ___ than the actual nuclear charge.

Answer 14

less

Question 15

Each step down in a group represents what in regards to the Zeff.

Answer 15

1. a large increase in the nuclear charge, Z

2. an additional shell of core electrons to shield the valence electrons from the nucleus.

Question 16

What are the two ways to define atomic radius?

Answer 16

1. Metallic radius

2. Covalent radius

Question 17

This is the atomic radius that is half the distance between the nuclei of two adjacent, identical metal atoms.

Answer 17

Metallic Radius

Question 18

This is the atomic radius that is half the distance between adjacent, identical nuclei in a molecule.

Answer 18

Covalent Radius

Question 19

What are the 2 atomic radius rules?

Answer 19

1. The atomic radius increases from top to bottom in a group.
2. It decreases as we move across a period from left to right.

Question 20

This is the minimum energy required to remove an electron from an atom in the gas phase. It is a measure of the strength from with which an atom holds onto its electrons.

Answer 20

Ionization Energy (IE)

Question 21

The first ionization energy is the removal of the most ____ held electron.

Answer 21

loosley

Question 22

The first ionization energy is the removal of the most ____ held electron.

Answer 22

loosley

Question 23

What are the 2 Ionization Energy rules?

Answer 23

1. The ionization energy decreases down a group.

2. It increases from left to right.

Question 24

___ electrons are generally more strongly bound from left to right in a period.

Answer 24

Valence

Question 25

This is the energy released when an atom is the gas phase accepts an electron, so it is the negative of the enthalpy change, delta H.

Answer 25

Electron Affinity

Question 26

What are the rule of electron Affinity?

Answer 26

It increases from left to right across a period, because it is easier to add negatively charged electrons as the positive charge of the elements nucleus increases.

Question 27

Which 2 groups do not form stable negative ions?

Answer 27

2A- alkali earth metals | 8A- Noble Gases

Question 28

It is important to write out orbital diagrams for the valence electrons in which type of problems?

Answer 28

Electron Affinity.

Question 29

It is more difficult in Electron Affinity to add an electron to a ____ occupied orbital than to an empty one.

Answer 29

partially

Question 30

These are characteristics of? 1. Shiny, lustrous, and malleable 2. Good conductors of heat and electricity 3. Low ionization energies (so they easily lose their valence electrons to form cations) 4. Form Ionic compounds with chlorine (metal chlorides) 5. Form basic compounds with oxygen (metal oxides)

Answer 30

Metals

Question 31

These are characteristics of? 1. Vary in color and lack shiny appearance. Dull 2. Brittle rather than malleable 3. Poor conductors of heat and electricity 4. Form acidic, molecular compounds with oxygen. 5. Have high electron affinities (commonly form anions when they accept electrons)

Answer 31

Non-Metals

Question 32

What are the 2 ionization energy rules of metals?

Answer 32

1. IE decreases going down a group | 2. IE increases from left to right

Question 33

What are the 2 rules of metallic characteristics?

Answer 33

1. Increase as you go down a group | 2. Decrease from left to right in a period

Question 34

The valence electron configurations of Noble Gases are extraordinarily ____.

Answer 34

Stable

Question 35

Other main group elements tend to either ___ or ___ a electrons to acheive the same number of electrons as the nearest noble gas.

Answer 35

Lose or Gain

Question 36

Species with identical electron configurations are called what?

Answer 36

Isoelectronic

Question 37

To write the electron configuration of an ion formed by a main group element, you must...

Answer 37

1. Write the configuration for the atom | 2. Add or remove the appropriate number of electrons

Question 38

An atom always loses electrons first from the shell with the highest value of ___. Therefore valence electrons are always lost first.

Answer 38

n

Question 39

When an atom gains or loses one or more electrons to become an ion, its radius changes.

Answer 39

Ionic Radius

Question 40

The ionic radius affects the ___ and ___ chemical properties of ionic compounds.

Answer 40

Physical and Chemical

Question 41

When an atom loses electrons and becomes a cation, its radius ____.

Answer 41

Decreases

Question 42

____ electrons lead to: A reduction in electron-electron repulsion and A reduction in shielding of the valence electrons and A higher Zeff.

Answer 42

Fewer

Question 43

A substantial ____ in radius occurs when all of an atoms valence electrons are removed. This is the case with ions of most main group elements which are isoelectronic.

Answer 43

decrease

Question 44

When an atom gains one or more electrons and becomes and anion its radius ____.

Answer 44

increases

Question 45

____ electrons leads to: Increased electron-electron repulsion and therefore A higher degree of shielding of the valence electrons and Lower Zeff.

Answer 45

Additional

Question 46

Ionic radius ____ going down a group as n increases.

Answer 46

increases

Question 47

This is a series of two for more species that have identical electron configurations but different nuclear charges.

Answer 47

isoelectronic series

Question 48

What is an example of an isoelectronic series?

Answer 48

O^2, F- and Ne. they all have 10 electrons

Question 49

In an isoelectronic series, the species with the ____ nuclear charge will have the largest radius. And species with the ____ nuclear charge will have the smallest radius.

Answer 49

smallest | largest