Chapter 8

Question 1

What is electron configuration?

Answer 1

Shows the particular orbitals that electrons occupy for an atom

Question 2

How do the arrows in an orbital diagram show the spin of the electron?

Answer 2

An arrow up shows +1/2

An arrow down shows -1/2

Question 3

What is the Pauli exclusion principle?

Answer 3

States that no two electrons in an atom can have the same four quantum numbers

Question 4

What does degenerate mean?

Answer 4

Orbitals that all have the same energy

Ex 3s 3p 3d orbitals all have same energy

Question 5

What is coulomb’s law?

Answer 5

Describes the attractions and repulsions between charged particles
States that the potential energy (E) of two charged particles depends on their charges (q1 and q2) and their separation (r)

Question 6

What is the equation of Coulomb’s law given energy of charged particles and their charges?

Answer 6

E=1/4piee0 (q1q2/r)

e0=constant
r=separation
Q1 and q2= their charges

Question 7

How is potential energy affected by like charges?

Answer 7

The potential energy is positive and decreases as the particles get further apart

Question 8

How is the potential energy affected by opposite charges?

Answer 8

The potential energy is negative and becomes more negative as the particles get closer together

Question 9

What is shielding in multielectron atoms?

Answer 9

The repulsion of one electron by other electrons

Question 10

What is penetration in atoms?

Answer 10

Bringing another electron so close to the nucleus that it penetrates the electron cloud and experiences the positive charge of the nucleus

Question 11

Which has lower energy the 1s orbital or the 1d orbital?

Answer 11

1s

Question 12

What is the Aufbau Principle?

Answer 12

The pattern of orbital filling

Electrons full atomic orbitals of the lowest available energy levels first

Question 13

What is Hund’s rule?

Answer 13

States that when filling degenerate orbitals, electrons fill them singly first, with parallel spins
The way of filling orbitals
All arrows up first then add arrows down

Question 14

What are valence electrons? How do you determine an atoms valence electrons?

Answer 14

Those in the outermost principal energy level

Use the electron configuration and the electrons of the highest n number it has are the valence electrons
1s2 2s2 2p6 3s2 3p2
4 valence electrons
Or by group number

Question 15

Why do we write the 3d orbital with the 4s orbital?

Answer 15

Because the 4s orbital is lower in energy than the 3d

Question 16

What are the special cases of electron configuration for CE and Cu?

Answer 16

Cr- 4s1 3d5

Cu- 4s1 3d10

Question 17

What determines the chemical properties of elements?

Example?

Answer 17

The number of valence electrons they contain
Ex: noble gases have full valence shell and are generally stable
Alkali metals are most reactive since they have 1 valence electron

Question 18

How is the binding atomic radius defined for metals and nonmetals?

Answer 18

Nonmetals- one half the distance between two of the atoms bonded together
Metals- one half the distance between two of the atoms next to each other in a crystal of the metal

Question 19

What is the trend in the periodic table for the atomic radii?

Answer 19

Decreases up and to the right of the table

Question 20

What is the formula for finding the effective nuclear charge?

Answer 20

Zeff=Z-S
Zeff= effective nuclear charge
Z= actual nuclear charge
S= charge shielded by other electrons

Question 21

What’s the difference between core electrons and outermost electrons in terms of shielding?

Answer 21

Core electrons efficiently shield electrons in the outermost principal energy level from nuclear charge
Outermost electrons do not efficiently shield one another from nuclear charge

Question 22

When changing the electron configuration of cations and anions what do you take electrons from first if you run out of an energy level?

Answer 22

THE NEXT HIGHEST N NUMBER NOT ENERGY LEVEL
EX: V (AR) 4s2 3d3
V2+ (Ar) 4s0 3d3

Question 23

What does paramagnetic mean?

Answer 23

If an atom or ion contains unpaired electrons it is attracted by an external magnetic field
One up arrow without a down arrow

Question 24

What does diamagnetic mean?

Answer 24

An atom or ion in what all electrons are paired and is not attracted to an external magnetic field
All up arrows with down arrows

Question 25

How are the sizes of atoms affected by cations and anions?

Answer 25

Cations are much smaller than their corresponding atoms

Anions are much larger than their corresponding atoms

Question 26

What does isoelectric mean?

Answer 26

Ions with the same number of electrons

Question 27

Why are not all isoelectric ions the same size?

Answer 27

Because some have more protons resulting in a stronger positive mass pulling on the same amount of electrons

Question 28

What is ionization energy? What is it’s trend across the periodic table?

Answer 28

The energy required to remove an electron
Always positive

Increases up the periodic table and to the right

Question 29

What is the difference between forst ionization and second ionization energy?

Answer 29

First is the energy to remove the first electron

Second is the energy to remove the second and is much larger

Question 30

What is the electron affinity? What is it’s trend on the periodic table?

Answer 30

The energy change associated with the gaining of an electron by the atom in gaseous state
Usually negative
Increases (negatively) to the right and up the periodic table

Question 31

What is metallic character? What is it’s trend on the periodic table?

Answer 31

The properties associated with metals

Decreases to the right and up the periodic table

Question 32

What is the rule when dealing with atomic radii with elements with the same amount of electrons?

Answer 32

The greater the ionic charge, the smaller the ionic radii