Metals

Question 1

What is Aufbau’s principle?

Answer 1

orbitals of lower energy get filled first

Question 2

What is Pauli’s exclusion principle

Answer 2

the maximum number of electrons per orbital is 2 and no two electrons in an atom or ion can have the same four quantum numbers

Question 3

What is Hund’s rule

Answer 3

When filling degenerate orbitals put one electron in each of the degenerate orbitals before pairing electrons

Question 4

e- come out the shell with the largest ____ ____ first

Answer 4

n value

could also say with the highest principle quantum number

Question 5

Name 6 general properties of metals

Answer 5

• Conductive of heat and energy
• malleable
• Ductile
• shiny
• hard (Na and Hg exceptions)
• high melting and boiling points

Question 6

What is ionization energy?

Answer 6

the energy required to remove an electron from the gaseous atom or ion

Question 7

Why is ionization energy low in metals?

Answer 7

electrons are already mobile within the metal and so can be removed from the structure easily

Question 8

Metals are made up of…?

Answer 8

closely packed metal cations in “a sea of electrons”

Question 9

In metals e- are ___ throughout the _____

Answer 9

delocalized

lattice

Question 10

Can you isolate ions?

Answer 10

no

Question 11

Are ions compounds?

Answer 11

no

Question 12

Cations are ____ than the atoms from which they

are formed

Answer 12

smaller

Question 13

Define isoelectronic

Answer 13

species have the same number of electrons in identical configurations

Question 14

For isoelectronic cations, the more positive the ionic charge, the ____ the ionic radius.

Answer 14

smaller

Question 15

Anions are ___ than the atoms from which they are formed.

Answer 15

larger

Question 16

For isoelectronic anions, the more negative the charge, the ____ the ionic radius.

Answer 16

larger

Question 17

Ionic bonding results from the reaction of an atom with ____ ionization energy with an atom of ____ electron affinity

Answer 17

low

high

Question 18

in covalent bonds atoms ____

Answer 18

overlap

Question 19

In metallic bonds, ____ ____ are lost and gained

Answer 19

valance electrons

e- jump from one atom to another

Question 20

What is the structure of an MX compound?

Answer 20

metal cations packed with anions into an ionic lattice

Question 21

In MX what do the M and X stand for?

Answer 21

M is for metal

X is for halogen

Question 22

Lattice energy is the energy required to ….?

Answer 22

separate the ions

Question 23

Name 4 properties of MX compounds

Answer 23

• hard and brittle
• high melting point
• dissolve in polar (ionizing) solvents
• do not conduct electricity as solids but do conduct electricity in molten or solution form

Question 24

why does the size of M and M+ increase down the group?

Answer 24

More shells as you go down

Question 25

Why does IE decrease moving down a metal group?

Answer 25

Because the size of the orbitals increase moving down a column making the valance e- easier to remove

Question 26

Metals become more ____ moving down a column

Answer 26

metallic

Question 27

Why do metals become more metallic moving down a column?

Answer 27

Because the valance e- are easier to remove because the atoms are larger

Question 28

What is ionic potential?

Answer 28

the ratio of metal cation charge (Z) to ionic radius (r) (ie Z/r)

Question 29

Ionic potential measures the ability to ____

Answer 29

polarize

Question 30

The smaller the metal cation and the ___ its charge density, the ___ it will polarize the electron cloud of the anion

Answer 30

higher | more

Question 31

IP (ionic potential) or Polarizing ability ____ down a group

Answer 31

decreases

Question 32

Why is NaCl water soluble when AgCl is not?

Answer 32

Na+ has noble gas configuration but Ag+ has 5s and 4d orbitals which are closer in energy and this results in more polarizing effect so the AgCl salt is hard to dissolve

Question 33

Are most MX compounds water soluble?

Answer 33

yes

Question 34

Do anions polarize cations or do cations polarize anions?

Answer 34

Cations polarize anions

Question 35

The anion that has more ___ and a ___ volume is more likely to get polarized

Answer 35

electrons | larger

Question 36

Cations with the noble-gas electronic configurations are ___ polarizing than those with non-noble gas electronic configurations

Answer 36

less

Question 37

The cation with the larger charge density is __ likely to polarize an anion

Answer 37

more

Question 38

What are the group 1 metals called?

Answer 38

alkali metals

Question 39

The ionization energy of the alkali metals ____ down the group

Answer 39

decreases

Question 40

Are alkali metals (group 1) dense?

Answer 40

no they are low density metals

Question 41

Why is the metallic bonding of group 1/alkali metals weak?

Answer 41

because only one valance e- contributes to metallic bonding

Question 42

Why are group1/alkali earth metals not very dense?

Answer 42

Because they have very weak metallic bonding which is cause by there only be one valance e- per atom to contribute to metallic bonding

Question 43

The reactivity of metal _____ down a group

Answer 43

increases

Question 44

The reaction between an group1/alkali metal and water results in....?

Answer 44

an alkaline solution of a metal hydroxide

Question 45

What alkali earth metal can be used for carbon dioxide scrubbing?

Answer 45

Na in NaOH

Question 46

Which are more reactive alkali/group 1 metals or alkaline earth/group 2 metals?

Answer 46

Alkali/group 1 metals

Question 47

Group 1 metals have ____(lower/higher) melting points than group 2 metals

Answer 47

higher

Question 48

Why do group 2 metals have higher melting points than group 1 metals?

Answer 48

Because group 2 metals have more valance e- to contribute to metallic bonding

Question 49

Do ionic compounds containing group 1 or group 2 metals have lower solubility in water?

Answer 49

ionic compounds containing group 2 metals have a lower solubility in water

Question 50

Why do ionic compounds containing group 2 metals have lower solubility in water than group 1 metals?

Answer 50

group 2 metals have a stronger cation-anion interactions (ie stronger metallic bonding)

Question 51

Are lattices of ions with similar or dissimilar charge densities more stable?

Answer 51

similar

Question 52

Why are group 2/alkaline earth metals less reactive than group 1/alkali metals?

Answer 52

Because for group 2/alkaline earth metals to reach noble gas configuration the must lose 2 e- not just one. (Have to overcome 2 IE)

Question 53

Group 2 metals have higher melting points than group 1 metals with one exception. Which metal is the one exception?

Answer 53

Magnesium

Question 54

What is the layer that forms on group 2 metals that stop the reaction with water from continuing called?

Answer 54

a metaloxide layer

Question 55

The ____ (lower/higher) the charge density the more polarizing the cation

Answer 55

higher

Question 56

Which group 1 metals can react with unlimited oxygen supply to form oxides?

Answer 56

all group 1 metals

Question 57

Which group 1 metals can react with unlimited oxygen supply to form peroxides?

Answer 57

all group 1 metals except lithium (Li)

Question 58

Which group 1 metals can react with unlimited oxygen supply to form superoxides?

Answer 58

all group 1 metals except lithium (Li) and Sodium (Na) | ie from Potassium (K) down forms superoxides