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IB Chem > Chemistry Topic 3 > Flashcards

Chemistry Topic 3 Flashcards

Periodic Table

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1
Q

How do you find the effective nuclear charge?

A

Atomic number - number of nonvalence electrons

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2
Q

What two factors cause the outer electrons to not experience the full nuclear charge?

A

Repulsion and shielding

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3
Q

What is the nuclear charge?

A

The atomic number

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4
Q

What is the trend for effective nuclear charge across a period?

A

The effective nuclear charge increases because the number of shielding electrons remains the same, but the nuclear charge increases

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5
Q

What is the trend for effective nuclear charge down a group?

A

The effective nuclear charge remains the same because the nuclear charge and number of shielding electrons both increase by 8

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6
Q

How do we find the atomic radius?

A

Atomic radius is half the distance between the nuclei of neighboring atoms
*Must be solved this way because electrons are in orbitals and their exact location is unknown

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7
Q

Cations are (smaller/larger) than their atoms

A

Smaller

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8
Q

Anions are (smaller/larger) than their atoms

A

Larger

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9
Q

Electron affinity

A

A measure in the change in energy when 1 mole of electrons is added to 1 mole of gaseous atoms to form gaseous ions

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10
Q

When the first electron is added in electron affinity, is the reaction endothermic or exothermic?

A

Exothermic

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11
Q

When does electron affinity become an endothermic process?

A

When a second electron is added because the anion and second electron repel

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12
Q

Electronegativity

A

A measure of an element’s attraction for an electron in a covalent bond/a bonding pair of electrons

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13
Q

Down group 1, do melting points increase or decrease? Explain why.

A

Melting points decrease because the atomic radius increases which makes it harder for the metallic bonds to reach the electrons in other atoms, so the IMFs are weaker, and it takes less energy to melt

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14
Q

Down group 17, do melting points increase or decrease? Explain why.

A

Melting points increase because atomic radius increases, so the strength of the temporary dipoles in London dispersion forces increases, so the IMFs are stronger, and it takes more energy to melt

Group 17s are diatomic, when size of molecules increases, LDFs increase

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15
Q

Metalloids and macromolecules (network solids) have ____ melting points

A

Very high

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16
Q

Metals have ____ melting points

A

High

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17
Q

Nonmetals have ____ melting points

A

Low

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18
Q

Noble gases have ____ melting points

A

Very low

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19
Q

Does reactivity for metals increase as you go up or down the groups?

A

Down

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20
Q

Does reactivity for nonmetals increase as you go up or down the groups?

A

Up

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21
Q

Group 1 metals react with halogens to form what?

A

Ionic salts

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22
Q

What do group 1 metals form when they react with water?

A

A base and hydrogen gas

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23
Q

When a group 1 reacts with water is the reaction endothermic or exothermic?

A

Exothermic

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24
Q

Metal oxides are (acidic/basic)

A

Basic

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25
Q

Nonmetal oxides are (acidic/basic)

A

Acidic

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26
Q

What products do an acid + base produce?

A

Water + a salt

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27
Q

What do metal oxides + water produce?

A

A base

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28
Q

What do nonmetal oxides + water produce?

A

An acid

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29
Q

P4O10 + _H20 -> _____

A

6H20; 4H3PO4

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30
Q

P4O6 + _H20 -> _____

A

6H20; 4H3PO3

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31
Q

SO3 + H20 -> _____

A

H2SO4

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32
Q

SO2 + H2O -> ____

A

H2SO3

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33
Q

Cl2O7 + H2O -> ____

A

2HClO4

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34
Q

Cl2O + H2O -> ____

A

2HClO

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35
Q

What is an amphoteric oxide and what is an example of one?

A

An oxide that can act as both an acid and a base. Al2O3

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36
Q

What is a Lewis acid?

A

Something that accepts an electron

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37
Q

What is a Lewis base?

A

Something that donates an electron

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38
Q

What color and phase is fluorine?

A

Yellow gas

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39
Q

What color and phase is chlorine?

A

Yellowish/green gas

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40
Q

What color and phase is bromine?

A

Dark red liquid

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41
Q

What color and phase is iodine?

A

Purple solid

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42
Q

In order for a displacement reaction to happen, the free element must be ____ than the element in the compound that its replacing

A

More reactive (higher up on the table for nonmetals)

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43
Q

For displacement reactions with halogens, the color that is seen is always determined by what?

A

The free element that isn’t in the compound

44
Q

What happens if the free element is less reactive than the element it is replacing in a displacement reaction?

A

No reaction or color change occurs

45
Q

What fact about the d sublevel do all transition elements have as atoms or ions?

A

They all have incomplete d sublevels

46
Q

Transition elements form _____ with ligands

A

Complex ions

47
Q

What two elements in the d-block aren’t transition elements in their atom and ion form?

A

Zinc/Zinc+2 and Copper/Copper+1

48
Q

What element in the d-block is not a transition element ONLY in its ion

A

Scandium (+3 ion)

49
Q

True or false: transition elements have catalyst and magnetic properties

A

True!

50
Q

Which two transition elements have high oxidation states, which makes them good oxidation agents down to +3 and +2?

A

Chromium and manganese

51
Q

List two examples of homogeneous catalysts

A

Fe+3 Heme in blood to transport oxygen, and Co+3 in vitamin B12

52
Q

What are the two possible heterogeneous catalysts in catalytic converters in cars, and what do they do?

A

Palladium and platinum (solids), and they reduce NO and CO production

53
Q

What is the name of the process that produces ammonia with the help of a catalyst, and what is that catalyst?

A

The Haber process, and solid iron is the heterogeneous catalyst

54
Q

What catalyst is used for a contact process production of sulfuric acid, and what is the equation of the reaction?

A

Vanadium (V) oxide (V2O5)
Equation: 2SO2(g) + O2(g) -> 2SO3(g)

55
Q

What is a hydrogenation reaction (equation and catalyst)?

A

C2H4(g) + H2(g) -> C2H6(g)
Where Nickel is the heterogeneous catalyst that turns an alkene into an alkane (makes an unsaterated hydrocarbon saturated)

56
Q

What is the decomposition of hydrogen peroxide (equation and catalyst)?

A

H2O2(aq) -> 2H2O(l) + O2(g)
Manganese (IV) Oxide (MnO2) is the catalyst

57
Q

Which group is more reactive, group 1 or group 2?

A

Group 1

58
Q

List the properties of paramagnetic things

A
  • Unpaired electrons
  • Pulled into a magnetic field
  • Do NOT retain magnetic properties after the field is removed
  • More unpaired electrons = more attraction
59
Q

List the properties of diamagnetic things

A
  • Paired electrons
  • Weakly repelled by magnetic field
  • Do NOT retain magnetic properties after the field is removed
60
Q

List the properties of ferromagnetic things

A
  • Unpaired electrons that align parallel to each other in domains
  • Retain magnetic properties when the magnetic field is removed
61
Q

What are Complex ions?

A

Transition metal ions, due to their small size, act as Lewis acids (are electron deficient) and attract species that are electron rich called ligands

62
Q

Are ligands Lewis acids or bases?

A

Bases

63
Q

What are Ligands?

A

Species with lone pair(s) of electrons that form coordinate covalent bonds with a central metal ion

64
Q

The _____ the oxidation states, the more likely to have covalent properties

A

higher

65
Q

List the spectrochemical series in order from weakest to strongest

A

I- < Cl- < F- < OH- < H2O < SCN- < NH3 < NO- < CN- = CO-

66
Q

What is a coordinate covalent bonds?

A

A bond where one element donates both electrons, and the other does nothing

67
Q

What is a monodentant ligand?

A

A ligand that forms one coordinate covalent bonds using one lone pair of electrons

68
Q

If the ligand is neutral, how do we find the charge of the central metal ion?

A

Its just whatever the charge of the complex ion is

69
Q

What is the charge of ammonia

A

Nothing!

70
Q

Coordination number

A

The number of coordinate covalent bonds formed from the ligand to the central metal ion

71
Q

Polydentate Ligands

A

Contain MORE THAN 1 pair of lone electrons and can form 2 or more coordinate covalent bonds to the metal ion

72
Q

Bidentant Ligands

A

Can form 2 coordinate covalent bonds

73
Q

Hexadentate Ligand

A

Has 6 atoms with lone pairs of electrons

74
Q

Chelates

A

2 or more separate coordinate covalent bonds between ligand and central atom

75
Q

What is the color of the transition metal related to?

A

The presence of partially filled d orbitals

76
Q

If a transition metal appears yellow, what color light is it absorbing?

A

Purple! - Always the complementary color on the color wheel

77
Q

Which three ions are always colorless and why?

A

Sc 3+
Zn 2+
Cu 1+
Because they do not have any partially filled d orbitals

78
Q

In a free ion, the d orbitals are all of _____ energy, so they are called _____

A

Equal; degenerate

79
Q

Where are the five d orbitals located?

A

3 are between the axis, and 2 are along the axis

80
Q

Why do the 2 d orbitals that are along the axis split apart from the other 3 when a ligand comes in?

A

The lone electron(s) in the ligand repel the orbitals

81
Q

The amount of _____ determines the color reflected in a complex ion

A

The amount of energy in the splitting

82
Q

List the four things that cause the splitting energy to change

A

Identity of central metal ion, oxidation state of metal ion, geometry of complex ion, and identity of ligand

83
Q

Do larger central metals provide greater or less splitting of the d orbitals?

A

Greater!

84
Q

Great amounts of splitting in the d orbitals = (high/low) energy = (high/low) frequency = (high/low) wavelength

A

High energy, high frequency, low wavelength

85
Q

In the same metal, as the oxidation state increases, does the splitting of the d orbitals increase or decrease?

A

Increase!

86
Q

How can you tell if the geometry of the complex ion is what’s changing the splitting in the d orbitals?

A

If the only difference is the number of Ligands

87
Q

How many ligands are attached in an octahedral complex ion? tetrahedral? linear?

A

6, 4, 2

88
Q

If there are more ligands attached in a complex ion, is there more or less splitting?

A

More Ligands = more splitting

89
Q

Stronger Ligand = (more/less) splitting

A

More!

90
Q

When some of the water ligands in a [Cu(H20)6]2+ ion are replaced with ammonia, does the splitting increase or decrease? Also, what color will the new ion be?

A

The splitting increases, and the new ion will be dark blue/violet

91
Q

If you were to arrange ions in order of largest radius to smallest, and they all have the same charge, which one would have the largest ionic radius?

A

Whichever one has the largest atomic radius

92
Q

Are elements Lu and Lr part of the d or f block?

A

d block

93
Q

Are elements La and Ac part of the d or f block?

A

f block

94
Q

Explain why there is a large increase in ionic radius from Si 4+ to P 3-

A

P 3- has another energy level

95
Q

Explain why sulfur has a higher melting point than phosphorus

A

Phosphorus has a greater atomic radius than sulfur, so sulfur atoms are more tightly held together, and therefore it takes more energy to break them apart

For individual atoms, small radius = strong IMFs

96
Q

Does a bigger molecule mean stronger or weaker London dispersion forces?

A

Stronger!

97
Q

What happens when a group 1 metal is added to water?

A

H2 is created, the temperature of the water increases, and a clear, colorless solution (a base) is formed (also it explodes)

98
Q

What does the spectrochemical series list?

A

Ligands in order of their ability to split the d orbitals of transition metals

99
Q

What are the products of a reaction between chlorine and water?

A

HCl and HOCl

Don’t really have to know this, just know that it should produce acids

100
Q

What is the maximum amount of orbitals in the n=2 energy level?

A

4 (1 from 2s, 3 from 2p)

101
Q

Are metalloids acidic or basic?

A

Acidic!

102
Q

What is an essential feature of a ligand?

A

The presence of a non-bonding pair of electrons

103
Q

If all the ions have the same number of electrons (but they’re different elements), how do you determine which one is the smallest and largest?

A

Whichever one has the most amount of protons is the smallest because it can pull the electrons in closer, and whichever has the least amount is the biggest

104
Q

What are the three ferromagnetic elements?

A

Iron, Cobalt, Nickel

105
Q

Can bromine oxidize iodine?

A

Yes! Br2 + KI -> I2 + KBr, so Iodine goes from being a -1 to a 0, so it is losing an electron

106
Q

Where do transition metals lose their first electron from?

A

The outermost s orbital

107
Q

When the valence electrons are closer to the nucleus, they are ____ likely to react

A

Less!

IB Chem (3 decks)

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