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CHEM 250 - UBC > Metals > Flashcards

Metals Flashcards

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1
Q

What is Aufbau’s principle?

A

orbitals of lower energy get filled first

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2
Q

What is Pauli’s exclusion principle

A

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

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3
Q

What is Hund’s rule

A

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

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4
Q

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

A

n value

could also say with the highest principle quantum number

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5
Q

Name 6 general properties of metals

A
  • Conductive of heat and energy
  • malleable
  • Ductile
  • shiny
  • hard (Na and Hg exceptions)
  • high melting and boiling points
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6
Q

What is ionization energy?

A

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

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7
Q

Why is ionization energy low in metals?

A

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

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8
Q

Metals are made up of…?

A

closely packed metal cations in “a sea of electrons”

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9
Q

In metals e- are ___ throughout the _____

A

delocalized

lattice

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10
Q

Can you isolate ions?

A

no

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11
Q

Are ions compounds?

A

no

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12
Q

Cations are ____ than the atoms from which they

are formed

A

smaller

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13
Q

Define isoelectronic

A

species have the same number of electrons in identical configurations

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14
Q

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

A

smaller

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15
Q

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

A

larger

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16
Q

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

A

larger

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17
Q

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

A

low

high

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18
Q

in covalent bonds atoms ____

A

overlap

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19
Q

In metallic bonds, ____ ____ are lost and gained

A

valance electrons

e- jump from one atom to another

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20
Q

What is the structure of an MX compound?

A

metal cations packed with anions into an ionic lattice

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21
Q

In MX what do the M and X stand for?

A

M is for metal

X is for halogen

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22
Q

Lattice energy is the energy required to ….?

A

separate the ions

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23
Q

Name 4 properties of MX compounds

A
  • 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
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24
Q

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

A

More shells as you go down

25
Q

Why does IE decrease moving down a metal group?

A

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

26
Q

Metals become more ____ moving down a column

A

metallic

27
Q

Why do metals become more metallic moving down a column?

A

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

28
Q

What is ionic potential?

A

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

29
Q

Ionic potential measures the ability to ____

A

polarize

30
Q

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

A

higher

more

31
Q

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

A

decreases

32
Q

Why is NaCl water soluble when AgCl is not?

A

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

33
Q

Are most MX compounds water soluble?

A

yes

34
Q

Do anions polarize cations or do cations polarize anions?

A

Cations polarize anions

35
Q

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

A

electrons

larger

36
Q

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

A

less

37
Q

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

A

more

38
Q

What are the group 1 metals called?

A

alkali metals

39
Q

The ionization energy of the alkali metals ____ down the group

A

decreases

40
Q

Are alkali metals (group 1) dense?

A

no they are low density metals

41
Q

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

A

because only one valance e- contributes to metallic bonding

42
Q

Why are group1/alkali earth metals not very dense?

A

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

43
Q

The reactivity of metal _____ down a group

A

increases

44
Q

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

A

an alkaline solution of a metal hydroxide

45
Q

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

A

Na in NaOH

46
Q

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

A

Alkali/group 1 metals

47
Q

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

A

higher

48
Q

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

A

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

49
Q

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

A

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

50
Q

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

A

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

51
Q

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

A

similar

52
Q

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

A

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)

53
Q

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

A

Magnesium

54
Q

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

A

a metaloxide layer

55
Q

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

A

higher

56
Q

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

A

all group 1 metals

57
Q

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

A

all group 1 metals except lithium (Li)

58
Q

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

A

all group 1 metals except lithium (Li) and Sodium (Na)

ie from Potassium (K) down forms superoxides

CHEM 250 - UBC (12 decks)

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