Chapter 5: Electronic Structure and Periodic Properties

Question 1

What is ionization energy?

Answer 1

The energy required to remove one electron from an atom

Question 2

The stability of an orbital can be determined by measuring?

Answer 2

The amount of ionization energy

Question 3

True or False: It is easy to remove an electron from a positive species?

Answer 3

False

Question 4

What is the screening effect?

Answer 4

The electron-electron repulsion canceled by the attraction to the nucleus

Question 5

Electrons are only screened by____electrons?

Answer 5

Inner

Question 5

True or False: The higher the value of the quantum number n, the more that orbital is screened by electrons in smaller, more stable orbitals?

Answer 5

True

Question 6

True/False: the higher the value of l, the less that orbital is screened by electrons in smaller, more stable orbitals?

Answer 6

False

Question 7

What factors control the energy of an orbital for most atoms?

Answer 7

The size and shape of the orbital

Question 8

Do the columns of elements contain similar chemical properties?

Answer 8

Yes

Question 9

What is the Pauli Exclusion Principle?

Answer 9

Each electron has a unique set of four quantum numbers; no two electrons can have the same set

Question 10

What is the Aufbau Principle?

Answer 10

The placement of electrons in orbitals starting with the lowest energy orbital

Question 11

What are the rules of Ground-State configurations?

Answer 11

1. Each electron occupies the most stable available orbital
2. No two electrons can have the same quantum numbers
3. Shell capacities : s: 2 electrons
   p: 6 electrons
   d: 10 electrons
   f: 14 electrons

Question 12

Accessible electrons are also called?

Answer 12

Valence electrons

Question 13

What is Hund’s rule?

Answer 13

The most stable configuration is the one with the maximum number of electrons with the same spin orientation

Question 13

What is noble gas configuration?

Answer 13

Specify the noble gas before the element and then write the remaining configuration

Question 13

What two elements don’t follow the regular progression of configuration? What is their configuration?

Answer 13

Cr: 4s1 3d5
Cu: 4s1 3d10

Question 14

What are near-degenerate orbitals?

Answer 14

Orbitals with nearly the same energy. Because the orbitals are so close in energy, it is possible for an electron to the promoted to the higher energy level

Question 15

Isoelectronic

Answer 15

Atoms and ions that have the same number of electrons

Question 16

For neutral atoms and anions, place electrons in _____ before ________

Answer 16

ns, (n-1)d

Question 17

For cations, place electrons in _____before_____

Answer 17

(n-1)d, ns

Question 18

Paramagnetic

Answer 18

Attracted to a magnet, aligns itself in a magnetic field

unpaired electrons

Question 18

Diamagnetic

Answer 18

Repelled by a strong magnet

Paired electrons (spin cancels out)

Question 19

Are paramagnetic materials weak or strong?

Answer 19

Weak

Question 20

Strong paramagnetic materials are called

Answer 20

Ferromagnetic

Question 21

The number of unpaired electrons in a paramagnetic substance can be measured with a____

Answer 21

Gouy balance

Question 22

What type of substance does paramagnetism occur in?

Answer 22

Ions or atoms with unpaired electrons

Question 22

What type of substance does diamagnetism occur in?

Answer 22

Ions or atoms that have paired electrons

Question 23

Atomic radii

Answer 23

The distance between the nucleus and outer surface of the largest orbital

Question 24

Electron affinity

Answer 24

The amount of energy released when an electron is added to a neutral atom to form an anion

Question 24

Ionization energy

Answer 24

Energy required to remove an electron from an atom in the gas phase

Question 25

As n increases, atomic orbitals____

Answer 25

Become larger and less stable

Question 26

As Z increases, atomic orbitals____

Answer 26

Become smaller and more stable

Question 27

What is Z?

Answer 27

Atomic number (number of protons)

Question 28

For the main group elements, the ionization energy increases___?

Answer 28

Going up and across the right of the periodic table

Question 29

Does electron affinity have a clear trend as n increases? What is the one general pattern?

Answer 29

No. Electron affinity tends to become more negative moving from the left to right across a row of the periodic table

Question 29

Zeff increases as the number of electrons____?

Answer 29

Decreases As the number of electrons decrease, each electron feels a greater electrical attraction to the nucleus, resulting in a larger ionization energy

Question 30

What are the irregularities in ionization energies?

Answer 30

1. Aluminium has a smaller ionization energy than either of its neighbours in Row 3 2. Oxygen has a smaller ionization energy than either of its neighbours in Row 2.

Question 31

The radius of a cation is always____than the corresponding atom

Answer 31

Smaller

Question 32

The radius of an anion is always ______ than the corresponding atom

Answer 32

Larger

Question 33

For isoelectronic species, as Z increases __________?

Answer 33

It becomes more difficult to remove an electron

Question 34

What is the vaporization and ionization of an atom to form a cation?

Answer 34

(s) -----> (g) + e- Esublimation= (+) E=IE= (+)

Question 35

Condensation of the two to form the solid salt

Answer 35

(+) + (-) ----> (s) (-)E lattice = (-)

Question 35

Bond breakage and ionization of atom to form an anion

Answer 35

(g) + e- ------> -(g) E=1/2BE= (+) E=EA= (-)

Question 36

Overall reaction

Answer 36

Add all of the energies together

Question 37

What is the Born-Haber cycle?

Answer 37

A series of steps involving ions in the gas phase

Question 38

What is lattice energy?

Answer 38

The energy released when an ionic solid decomposes into gaseous ions

Question 39

What does the magnitude of lattice energy depend on?

Answer 39

The charges of the ions, their size, and lattice arrangement

Question 39

Are ions formed by removing core electrons found in stable ionic compounds?

Answer 39

No

Question 40

What are halides?

Answer 40

When halogens react with metals to form binary compounds. They contain metal cations and halide anions

Question 40

Isolated atomic anions with charges more negative than -1 are always unstable except for _____?

Answer 40

O2- and S2-

Question 41

What are the trends in lattice energy?

Answer 41

1. Lattice energy will increase as ionic charge increases and will decrease as ionic size increases 2. Lattice energy is the sum of all ion interactions in the solid ionic compound