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Chemistry > Chemistry - bonding > Flashcards

Chemistry - bonding Flashcards

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1
Q

Ionic bonds are formed between a…

A

metal and a non metal atom.

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2
Q

Covalent bonds are formed between two

A

nonmetal atoms or between a nonmetal and hydrogen

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3
Q

Lewis diagrams help us to visualise electrons in the….

A

outer energy levels of atoms.

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4
Q

Bonded pairs of electrons are

A

the electrons pairs that get shared between two atoms.

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5
Q

Unbonded pairs of electrons are called

A

lone pairs.

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6
Q

Shapes of molecules: (linear)

A

Any molecule with only two atoms bonded together. Regardless of weather any lone pairs exist or not….The bond angle is 180°

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7
Q

VSEPR theory (linear bonded pairs)

A

Linear shapes molecules have repulsion between the bonded pairs of electrons. The bonded pairs arranged in a linear shape to minimise repulsion.

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8
Q

Bent or V-Shaped explanantion

A

There are four areas of electron densities around the central atom. Two of which are binding pairs and two lone pairs of electrons have a bent or v shape. Bond angle is 109°

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9
Q

VSEPR theory bent or (v-shaped)

A

There is repulsion between the bonded pairs of electrons and also between the bonded and lone pairs of electrons. The lone pairs repel the bonded pairs more. The molecules arranged in a bent shape to minimise repulsion.

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10
Q

Bent shaped - SO2 shape

A

A bent or v-shape can also be produced by a molecule with 3 areas of electron density. There are two bonding pairs and one lone pair around the centre sulphur. The bond is 120°C

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11
Q

Explain why water and sulphur dioxide have the same shape but different bond angles.

A

The central atom in sulphur dioxide has only one lone pair, as opposed to the two lone pairs on the central oxygen in water, there is decreased repulsion in sulphur dioxide a bond angle of approximately 120°C

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12
Q

Trigonal pyramid shape

A

A molecule with 4 areas of electron density has a tetrahedral arrangement, however, with 3 bonding pairs and one lone pair of electrons.

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13
Q

VSEPR theory (trigonal pyramid)

A

There is repulsion between the bonded pairs of electrons and also between the bonded and lone pairs. The molecule is arranged in a Trigonal pyramid shape to minimise repulsion. Bond angle 107.3°C

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14
Q

Triangular Planar shape

A

A molecule with three areas of electron density around the central atom where all are bonding pairs the molecule has a triangular planar shape.

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15
Q

VSEPR theory (triangular planar)

A

There is equal repulsion between the bonded pairs of electrons. The molecule arranges in a trigonal planar shape to minimise repulsion.

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16
Q

Tetrahedral shape

A

A molecule with four areas of electron densities where all of them are bonding pairs produces a tetrahedral in shape.

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17
Q

VSEPR theory (tetrahedral)

A

There is equal repulsion between the bonded pairs of electrons. The molecule arranged in a tetrahedral shape to minimise repulsion

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18
Q

Electronegativity

A

The tendency of an atom to attract a pair of electrons in a covalent bond

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19
Q

The polarity of a molecule depends on

A

the difference in electronegativities of the atoms in the molecules.

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20
Q

Non polar covalent bonds

A

A bond between two nonmetal atoms that have the same electronegativity value and therefore have equal sharing of the bonding electron pair.

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21
Q

Polar covalent bond

A

A bond between two nonmetal atoms that have different electronegativities and therefore have unequal sharing of the bonding electron pair.

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22
Q

Dipole

A

difference in electronegativity between two atoms.

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23
Q

Polar Molecule

A

A molecule in which the bond dipoles are present and there is uneven distribution of charge around the central atom.

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24
Q

Intramolecular Forces

A

occur within molecules. These are covalent bonds and are very strong.

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25
Q

Intermolecular Forces

A

attractive and repulsive forces that occur between molecules of a substance.

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26
Q

Intermolecular forces (vander waal forces.) (3)

A
  1. Temporary dipole-dipole attractions (weakest type of attraction) Found in all molecules.
  2. Permanent dipole-dipole attractions
  3. Hydrogen bonding (strongest type of attraction)
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27
Q

Solubility of polar and nonpolar liquids (2)

A
  1. Rules: “like dissolves like”
    Polar liquids are generally soluble in other polar liquids
  2. Non-polar liquids are generally soluble in non-polar solvents
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28
Q

Why are Non-polar liquids generally soluble in non-polar solvents

A

This is because the intermolecular forces between the two molecules must be of the same magnitude to allow one liquid to be soluble in another.

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29
Q

Molecular solids are made up of atoms….

A

covalently bonded together forming molecules.

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30
Q

Molecular substances are held together…..

A

intermolecular bonding

31
Q

Do molecular solids conduct electrcity

A

Molecular solids do not conduct electricity because they do not have free valence electrons or ions to carry the charge.

32
Q

Iodine and cyclohexane. (polarity and intermolecular forces)

A

Iodine mixes in cyclohexane as both are non polar molecules. The intermolecular forces between the two molecules is one of the same magnitude and they are broken and formed again to allow iodine to be soluble in cyclohexane.

33
Q

Ionic solids are composed of

A

cations and anions held together by ionic forces in a rigid lattice structure.

34
Q

Ionic bonding

A

refers to the electrostatic attraction between cations and anions. Ionic bonds are strong in nature.

35
Q

Physical properties of ionic solids
High melting points:

A

due to a large amount of energy is needed to overcome strong ionic bonds.

36
Q

Physical properties of ionic solids
Conductivity

A

in a solids state it does not conduct electricity because the ions cannot move out of the lattice structure.

37
Q

Is ionic solid aqueous?

A

Aqueous solution (dissolved in water) - it conducts because the ions can move carrying the charge.

38
Q

Physical properties of ionic solids:
Hardness and brittleness

A

when stress is applied to an ionic lattice the layers shift slightly. When they do ions of the same charge are brought close together. These repel and the structure breaks down into smaller pieces.

39
Q

Physical properties of ionic solids:
solubility

A

Ionic solids do not dissolve in non-polar solvents which have no charges, there are no attractions between the charged particles in the solid and the non charged particles in the solvent.

40
Q

Physical properties of ionic solids:
dissolving in water….

A

Ionic solids are soluble in water as the polar water molecules are attracted towards the ions from the lattice.

41
Q

The negatively charged end of the solvent molecules (water) get attracted to….

A

the positively charged cations.

42
Q

The positively charged end of the solvent molecule (water) gets attracted to….

A

the negatively charged anions.

43
Q

If the forces of attraction between an ion and the solvent molecules (water) is greater than the force of attraction between the ions themselves (ionic bonds)…

A

the solid dissolves

44
Q

The ions are then held in the solution being surrounded by…

A

the solvent molecules.

45
Q

What type of particle is in molecular solid

A

Molecules

46
Q

What type of particle is in ionic solids

A

Ions

47
Q

Type of attractive forces in molecules

A

intermolecular forces

48
Q

Type of attractive forces in ionic solids

A

Ionic bonds

49
Q

Property of molecular solid (2)

A

Low melting point
Does not conduct electricity

50
Q

Property of ionic solids (4)

A
  • High melting point
  • Brittle
  • Not conduct electricity in solid state
  • Conducts electricity when in molten aqueous.
51
Q

Diamond properties

  1. Hard?
  2. Conduct electricity
  3. Type of bond?
  4. Diamond made up of atoms…
A

Hard
Does not conduct electricity
All atoms are held together by strong covalent bonds
Diamond is made of atoms. All the atoms are held in place by strong covalent bonds; there are no free electrons. (free charge carries)

52
Q

Graphite properties
1. Hard?
2. Bonds?
3. Why does graphite conduct electricity?

A

1.Soft
2.Each carbon only has 3 bonds there are weak forces between the layers and the layers can slide
3.Graphite does conduct electricity because there are delocalised electrons which are free to move between the layers.

53
Q

A chemical reaction is always accompanied by a change in…

A

energy

54
Q

When chemical reactions occur new chemical bonds are….

A

formed between reactants and existing chemical bonds have to be broken.

55
Q

Exothermic reactions definition

A

When bonds are broken energy is released to surroundings. The test tube becomes warm and there is a rise in temperature.

56
Q

Endothermic reactions definition

A

When bonds are broken energy is needed. Reaction absorbs energy from the surroundings. The test tube feels cold as there is a decrease in temperature.

57
Q

Metallic solid are made up one type of..

A

metal atoms.

58
Q

The bond which exists between metal atoms is called

A

metallic bond

59
Q

Metallic solid structure

A

The atoms have released their valence electrons to become positive ions.
The metallic bond is the electrostatic attraction between the positive ions and the delocalised electrons.

60
Q

Metallic solid High melting point and boiling point

A

metals have high melting and boiling points because of the strong metallic bond.
Large amount of energy is needed to overcome the strong metallic bonds.

61
Q

Metallic solid: Malleable and ductile

A

The delocalised electron in the ‘sea of electrons’ in the metallic bond, enables the metal atoms to roll over each other when stress is applied. This is because the bonds are not directional.

62
Q

Metallic solid: lustre

A

When delocalised electrons come in contact with light, they vibrate. As a result, the electrons gain a small amount of energy and when this energy is released the surface and the metal shines.
Metal absorbs light energy and are able to reflect light of different wavelengths.

63
Q

Metallic solid: Conductivity
Electricity

A

The delocalised electrons carry the charge which allows it to conduct electricity.

64
Q

Metallic solid: Conductivity heat

A

When delocalised electrons carry energy this allows metal to conduct heat.

65
Q

what is the unit for mass

A

grams (g)

66
Q

What is the unit for moles (n)

A

mol

67
Q

What is the unit for molar mass

A

gmol-1

68
Q

Thermochemical calculations steps
(4)

A
  1. Calculate the moles (n) given the mass of the substance.
  2. Determine how many moles of the substance gives the △rH for the equation.
  3. Multiply the number of moles of substance in 1 by the △rH and divide by moles in 2 find the energy released or absorbed.
  4. State whether the amount of energy was released or absorbed.
69
Q

Bond energy or bond dissociation energy is…

A

the energy required to break one mole of a specified bond in a gaseous molecule.

70
Q

Bond energies (enthalpies) are….

A

positive. It is an endothermic reaction.

71
Q

Combustion of methane reaction…..

A

CH4(g) + 2O2 → 2H2O + CO2(g)

72
Q

Bonding breaking - endothermic or exothermic?

A

Energy is always required to break a bond. Bond breaking is always endothermic.

73
Q

Bond making - endothermic or exothermic

A

Energy is always released when a bond is formed. Bond making is always endothermic.

74
Q

Bond energy calculations formula

A

△rH = ∑ E (bonds broken) - ∑ E (bonds formed)

Chemistry (3 decks)

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