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NEW Spec Chemistry AS > Module 2 > Flashcards

Module 2 Flashcards

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1
Q

What does the mass number of an atom tell you about the sub-atomic particles?

A

Number of neutrons and protons.

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2
Q

What does the atomic number tell you about the sub-atomic particles?

A

Number of protons.

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3
Q

What is located in the centre of an atom?

A

Protons and neutrons.

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4
Q

What is the centre of an atom called?

A

Nucleus

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5
Q

What is the relative charge and mass of a proton?

A

Charge: +1
Mass: 1

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6
Q

What is the relative charge and mass of a neutron?

A

Charge: 0
Mass: 1

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7
Q

What is the relative charge and mass of an electron?

A

Charge: -1
Mass: 1/2000

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8
Q

Which sub-atomic particle changes when ions are formed?

A

Electrons

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9
Q

What type of ion will form when electrons are lost?

A

Positive ion

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10
Q

What type of ion will form if electrons are gained?

A

Negative ion

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11
Q

What is the definition of relative isotopic mass?

A

The mass of an atom of an isotope compared with 1/12th the mass of an atom of carbon-12.

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12
Q

What is the definition of relative atomic mass?

A

The weighted mean mass of an atom of an element compared with 1/12th the mass of an atom of a carbon-12.

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13
Q

What is the formula and charge of the carbonate ion?

A

CO3, 2-

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14
Q

What is the formula and charge of the sulphate ion?

A

SO4, 2-

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15
Q

What is the formula and charge on the hydroxide ion?

A

OH, -

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16
Q

What is the formula and charge on the ammonium ion?

A

NH4, 1+

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17
Q

What is the formula and charge on the nitrate ion?

A

NO3, 1-

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18
Q

What is the charge on a zinc ion?

A

2+

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19
Q

What is the charge on a silver ion?

A

1+

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20
Q

What does the group number from the Periodic Table tell you about an atom?

A

Number of outer electrons.

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21
Q

What are the units for amount of substance?

A

Mole (mol)

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22
Q

What is the equation for calculating the number of atoms/particles/molecules?

A

Number of particles = moles x Avogadro’s number

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23
Q

What is the equation for calculating mass?

A

Mass = Mr x mole

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24
Q

What is the equation for calculating concentration?

A

Concentration = moles/volume

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25
Q

What is the equation for calculating volume of a gas?

A

Volume = moles x 24 (in dm3)

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26
Q

What is the definition of an anhydrous salt?

A

A salt that contains no water molecules.

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27
Q

What is the definition of a hydrated salt?

A

A crystalline salt containing water molecules.

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28
Q

What is the definition for water of crystallisation?

A

Water molecules that form an essential part of the crystalline structure of a compound.

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29
Q

What is the ideal gas equation?

A

pV = nRT

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30
Q

When can atom economy be 100%?

A

When only one product is formed.

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31
Q

What are some of the reasons why percentage yield may not be 100%?

A
  1. Reaction may not go to completion.
  2. By-products may form.
  3. Impurities
  4. Some product/reactants can be left in apparatus.
  5. Purifying products can lead to loss.
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32
Q

How can atom economy for a reaction be increased?

A

Finding a use for by-products.

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33
Q

What is the formula of hydrochloride acid?

A

HCl

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34
Q

What is the formula of nitric acid?

A

HNO3

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35
Q

What is the formula of sulphuric acid?

A

H2SO4

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36
Q

What is the formula of ethanoic acid?

A

CH3COOH

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37
Q

What is the definition of an isotope?

A

Atoms of the same element with different numbers of neutrons (different mass number).

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38
Q

What is meant by the term strong acid?

A

A proton donor which fully dissociates.

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39
Q

What is meant by the term weak acid?

A

A proton donor which only partially dissociates.

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40
Q

What types of compounds are considered to be bases?

A

Metal hydroxides, metal oxides, ammonia

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41
Q

What is the formula of ammonia?

A

NH3

42
Q

What is the reaction equation for neutralisation?

A

H+ + OH- –> H2O

43
Q

What is the generic equation for forming a salt from a carbonate?

A

Acid + carbonate –> salt + water + carbon dioxide

44
Q

What is the generic equation for forming a salt from a base/alkali?

A

Acid + base –> salt + water

45
Q

What is the generic equation for forming a salt from a metal?

A

Acid + metal –> salt + hydrogen

46
Q

What is the oxidation number for an uncombined element?

A

Zero

47
Q

What is the oxidation number for combined oxygen (not in a peroxide or with F)?

A

-2

48
Q

What is the oxidation number for oxygen in a peroxide?

A

-1

49
Q

What is the oxidation number of oxygen when combined with F?

A

+2

50
Q

What is the oxidation number for combined hydrogen?

A

+1

51
Q

What is the oxidation number for hydrogen in metal hydrides?

A

-1

52
Q

What is the oxidation number of simple ions?

A

Charge on the ion

53
Q

What is the oxidation number of combined fluorine?

A

-1

54
Q

What needs to happen to the oxidation numbers for a neutral compound?

A

Add up to zero

55
Q

What do the Roman numerals in compound names indicate?

A

Charge on element of oxidation number of element

56
Q

What does the term oxidation mean?

A

The loss of electrons, loss of hydrogen, gain of oxygen or an increase in oxidation number.

57
Q

What does the term reduction mean?

A

The gain of electrons, gain of hydrogen, loss of oxygen or a decrease in oxidation number.

58
Q

How many electrons does the first shell hold?

A

2

59
Q

How many electrons does the second shell hold?

A

8

60
Q

How many electrons does the third shell hold?

A

18

61
Q

How many electrons does the fourth shell hold?

A

32

62
Q

What is the definition of an atomic orbital?

A

A region of space where it is likely that you will find two electrons, with opposite spins.

63
Q

What is the shape of the s-orbital?

A

Spherical

64
Q

What is the shape of the p-orbital?

A

Dumbbell

65
Q

How many orbitals are there in an s-sub-shell?

A

1

66
Q

How many orbitals are there in a p-sub-shell?

A

3

67
Q

How many orbitals are there in a d-sub-shell?

A

5

68
Q

What is special about the 4s orbital?

A

It fills and empties first (before the 3d).

69
Q

What is the definition of ionic bonding?

A

The electrostatic attraction between oppositely charged ions.

70
Q

How are ionic bonds formed?

A

Ions form from the loss and gain of electrons.

71
Q

What type of structure are ionic compounds?

A

Giant lattice

72
Q

Why do ionic compounds have high melting and boiling points?

A

Only strong electrostatic forces of attraction within the giant structure.

73
Q

Why do ionic compounds conduct when molten or in solution?

A

Ions are mobile

74
Q

Why are ionic compounds soluble in polar solvents?

A

The polar solvents attract the oppositely charged ions and pull the lattice apart. The larger the charges on the ions in the lattice the less soluble the compound.

75
Q

What is the definition of covalent bonding?

A

Electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms.

76
Q

What type of structure can covalent compounds have?

A

Simple or giant

77
Q

Which elements take part in giant covalent compounds?

A

Carbon and silicon

78
Q

Why do diamond and graphite have high melting and boiling points?

A

Only strong covalent bonds between atoms within the giant structure - diamond. Graphite has mostly strong bonds but with some weak intermolecular forces between layers.

79
Q

Why do simple covalent structures have low melting and boiling points?

A

Weak intermolecular forces between molecules which are being overcome.

80
Q

Why do most covalent compounds not conduct?

A

No mobile ions or delocalised electrons

81
Q

What is meant by the term dative covalent bond?

A

A covalent bond formed where both electrons in the shared pair are donated by one atom.

82
Q

What is the shape and bond angle in a molecule with 1 pair of bonded electrons and no lone pairs?

A

Linear, 180 degrees

83
Q

What is the shape and bond angle in a molecule with 2 pairs of bonded electrons and no lone pairs?

A

Linear, 180 degrees

84
Q

What is the shape and bond angle in a molecule with 3 pairs of bonded electrons and no lone pairs?

A

Trigonal planar, 120 degrees

85
Q

What is the shape and bond angle in a molecule with 2 pairs of bonded electrons and 2 lone pairs?

A

Non-linear (bent, v-shaped), 104.5 degrees

86
Q

What is the shape and bond angle in a molecule with 3 pairs of bonded electrons and 1 lone pair?

A

Pyramidal, 107 degrees

87
Q

What is the shape and bond angle in a molecule with 4 pairs of bonded electrons and no lone pairs?

A

Tetrahedral, 109.5 degrees

88
Q

What is the shape and bond angle in a molecule with 5 pairs of bonded electrons and no lone pairs?

A

Trigonal bipyramidal, 120 and 90 degrees

89
Q

What is the shape and bond angle in a molecule with 6 pairs of bonded electrons and no lone pairs?

A

Octahedral, 90 degrees

90
Q

What type of electrons repel the most?

A

Lone pairs (repel more than bonded pairs)

91
Q

What is the definition of electronegativity?

A

A measure of the attraction of an electron in a covalent bond.

92
Q

What does the Pauling value tell you about an element?

A

The strength of its electronegativity. Greater the value, the more electronegative.

93
Q

What does it mean for a bond to be polar?

A

A covalent bond that has a permanent dipole due to a difference in electronegativity between bonded atoms.

94
Q

What is needed for a molecule to be polar?

A

Polar bonds which do not cancel out due to symmetry.

95
Q

What leads to intermolecular forces?

A

Constant random movement of electrons.

96
Q

How are London (dispersion) forces formed?

A
  1. Movement of electrons leads to unbalanced distribution.
  2. Instantaneous dipole forms in the non-polar molecule.
  3. This induces a dipole in a neighbouring molecule.
  4. Weak attraction between the molecules.
97
Q

What are the 3 examples of Van dear Waals’ forces?

A
  1. Permanent dipole - induced dipole
  2. Permanent dipole - permanent dipole
  3. London forces
98
Q

What is meant by the term hydrogen bonding?

A

Permanent dipole - permanent dipole attraction between the hydrogen on a OH, NH or FH on one molecule and a lone pair on NOF of a different molecule.

99
Q

How does hydrogen bonding explain why ice is less dense than water?

A

Forms an open lattice with hydrogen bonds holding the water molecules apart.

100
Q

How does hydrogen bonding explain why water has a higher melting and boiling point than expected?

A

Hydrogen bonds are stronger than other intermolecular forces meaning more energy is needed to overcome them.

NEW Spec Chemistry AS (4 decks)

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