Chapter 7

Question 1

What is effective nuclear charge?

Answer 1

the attractive force between electron and the nucleus

Question 2

What does effective nuclear charge depend on?

Answer 2

depends on the magnitude of the nuclear charge and on the average distance between the nucleus and the electron

Question 3

What happens to the force as the nuclear charge increases?

Answer 3

increases

Question 4

What happens to the distance as nuclear charge increases?

Answer 4

moves farther from the nucleus

Question 5

What do electrons in many electron atoms do to each other?

Answer 5

screened from the nucleus by the other electrons

Question 6

What is the net attraction like for an atom that has more electrons than protons?

Answer 6

the net attraction is samller than it would experience in the absence of other electrons

Question 7

IS effective nuclear charge greater or smaller than nuclear charge?

Answer 7

smaller

Question 8

How do you find effective nuclear charge?

Answer 8

Zeff=Z-S

Question 9

What happens to effective nuclear charge as l increases?

Answer 9

increases

Question 10

What is the trend for effective nuclear charge?

Answer 10

increases left to right across a period

Question 11

Why does effective nuclear charge increase across the period?

Answer 11

number of protons increase which causing the energy to increase which means the screening off the electrons are inefftive

Question 12

What happens to effective nuclear charge going down a column?

Answer 12

effective nuclear charge icnreases slightly

Question 13

Why does effective nuclear charge increases as we go down a group?

Answer 13

the more diffuse core electron cloud is less table to screen the valence electron from the nuclear charge

Question 14

What is atomic radius?

Answer 14

an estimate of the size of an atom

Question 15

What is bonding atomic radius

Answer 15

the radius of an atom by the distances separating it from other atoms to which it is chemically bonded

Question 16

How do you find bonding atomic radius?

Answer 16

atomic radius x 1/2

Question 17

What does bonding atomic radii do as you go across a period?

Answer 17

decrease

Question 18

What does bonding atomic radii do as you go down a group?

Answer 18

increases

Question 19

Why does the bonding atomic radii increase as you go down a group?

Answer 19

increase in the quantum number(n) of the outher electrons. the probablitly of being farther from the nucleus

Question 20

Why does the bonding atomic radius tend to decrease across a period?

Answer 20

increase in Zeff across a period. draws the valence electrons closer to the nucleus

Question 21

How do you determine ionic radii?

Answer 21

interatomic distances in ionic compounds

Question 22

What does ionic radii depend on?

Answer 22

nuclear charge, the number of electrons, and the orbitals which the valence electrons reside

Question 23

Are cations smaller or larger then there parent electrons?

Answer 23

smaller

Question 24

Why are cations smaller then there parent atoms?

Answer 24

the number of electron-electron repulsions is reduced

Question 25

Are anions bigger or smaller then there parent atoms?

Answer 25

bigger

Question 26

Why are anions bigger then there parent atoms?

Answer 26

electrons are added to an atom, causing increased electron-electron repuslions

Question 27

What does ionic radius do as you go down a group?

Answer 27

increases

Question 28

What is an isoelectronic series?

Answer 28

a series of atoms, ions or molecules having the same number of electrons

Question 29

What does ionic radius d as nuclear charge increases?

Answer 29

decreases

Question 30

What is ionization energy?

Answer 30

the minimum enery required to remove an electron from the ground state of an isolated gaseous atom or ion

Question 31

What is electron Affinity?

Answer 31

the energy change that occurs when an electron is added to a gaseous atom or ion

Question 32

does ionization from a cation or an anion?

Answer 32

cation

Question 33

When ionization occurs does it jump to another energy level or does it drop another energy level?

Answer 33

jump to antoher energy level

Question 34

As ionization increases is it easier or harder to remove an electron?

Answer 34

harder

Question 35

As ionization increases does the energy increase or decrease?

Answer 35

increase

Question 36

What does the first ionization energy do as you go across a period?

Answer 36

increases

Question 37

What does ionization energy do as you go down a group?

Answer 37

decreases

Question 38

What does ionizaition energy measure?

Answer 38

when an atom loses an electron

Question 39

What does electron affinity measure?

Answer 39

the energy change when an atom gains an electron

Question 40

What causes electron affinity to increase(become more negative)

Answer 40

the greater the attraction between an atom and an added electron

Question 41

What part of the periodic table has the most negative electron affinities?

Answer 41

noble gases

Question 42

What part of the perioidc table is the most positive electron affinity?

Answer 42

halogens

Question 43

What does electron affinity do as you go across a period?

Answer 43

increases(become more negative)

Question 44

What does electron affinity do as you go down a group?

Answer 44

generally increases(become more negative