Chapter 7

Question 1

As we go Bottom-Up on the Periodic Table, the radius _____.

Answer 1

Decreases

Question 2

As we go right to left on the Periodic Table, the radius of the atom ______

Answer 2

Increases

Question 3

Positive ions are _____ than their neutral atoms.

Answer 3

Smaller

Question 4

Negative ions are _____ than their neutral atoms.

Answer 4

Bigger

Question 5

What is the isoelectronic series?

Answer 5

formed by ions that possess the same number of electrons.

Question 6

Ionic size _____ with an _____ nuclear charge

Answer 6

Decreases, increases

Question 7

What is ionization energy?

Answer 7

The amount of energy that is required to remove an electron from the ground state of a gaseous atom or ion.

Question 8

If IE is ____, it is difficult to remove an e-.

Answer 8

high

Question 9

If IE is ___, it’s not difficult to remove an atom.

Answer 9

low

Question 10

What are valence electrons?

Answer 10

An electron that is associated with an atom, and that can participate in the formation of a chemical bond.

Question 11

What is electron affinity?

Answer 11

The energy change (ΔE) accompanying the addition of an e- to a gaseous form. Most are negative.

Question 12

Typically, as you go left to right or down to up on the Periodic Table, electronic affinity becomes more __________.

Answer 12

Exothermic, though this pattern is not consistent.

Question 13

Characteristics of metals

Answer 13

Shiny, malleable, ductile, conductive of heat and electricity, high melting point, low ionization energy

Question 14

A metal to a nonmetal bond is referred to as a _____ compound

Answer 14

ionic

Question 15

A ________ to ________ bond is usually referred to as a molecular bond

Answer 15

nonmetal, nonmetal.

Question 16

Characteristics of nonmetals

Answer 16

Not shiny, poor conductivity, generally low melting points, easily gained electrons (favorable electron affinity)

Question 17

Nonmetal oxides are generally ______

Answer 17

acidic

Question 18

Characteristics of metalloids

Answer 18

Display intermediate properties (somewhat metal, somewhat nonmetal), shiny but not brittle, semiconductors

Question 19

If Ionization Energy is high, then it is _________ to remove an electron

Answer 19

difficult

Question 20

______ atoms have a lower Ionization Energy

Answer 20

Larger

Question 21

With transitions metals, as electrons are removed from the _ shell and then the _ shell

Answer 21

S, P

Question 22

In other metals and nonmetals, the _ orbital electrons disappear first

Answer 22

D

Question 23

The ionization required to remove an electron from an atom is always __

Answer 23

+

Question 24

If IE is high, that means it is _________ to remove the electron

Answer 24

difficult

Question 25

Exceptions to IE Rule on the PTE

Answer 25

Higher IE in 2A than 3A due to orbitals and atomic radius,

Higher IE in 5A than 6A because of the double orbitals being filled and having more shielding.

Question 26

More Electron Affinity means having __ energy, because the addition of e- is more __________

Answer 26

• because adding an electron is an exothermic reaction.

Question 27

Exceptions to the electron affinity rules:

Answer 27

Noble gases which require more energy to add electrons because they are already stable and do not require more electrons.

Question 28

Other exceptions to electron affinity:

Answer 28

1A and 2A, where any added e- must go into the P orbital

Question 29

Last exception to EA

Answer 29

No empty orbital, e- goes in occupied orbital causing repulsion