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Higher Chemistry > Jotter 1 > Flashcards

Jotter 1 Flashcards

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1
Q

What are halogens, where are they found in the periodic table and how does their reactivity decrease?

A

They are very reactive group 7 non-metals whose reactivity decreases going down the group.

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2
Q

What do alkali metals do to water?

A

Make the water alkaline.

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3
Q

What are atoms made up of?

A

Atoms are made up of a proton and a neutron which make up the nucleus and electrons which orbit the nucleus creating a shell.

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4
Q

What does the number of protons never do?

A

It never changes when looking at chemical change.

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5
Q

What is the group?

A

The group is the amount of electrons that the elements have in the outer layer.

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6
Q

As metals don’t have a group how are they written down in formulas?

A

A metal will always be given a valency in the formula.

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7
Q

What are the diatomic elements?

A

Hydrogen, Nitrogen, Oxygen, Bromine, Iodine, Chlorine, Fluorine.

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8
Q

What is the atomic size of an element?

A

The atomic size is the diameter/size of the atom.

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9
Q

How does the atomic size decrease?

A

Atomic size decreases due to an increase in nuclear charge on the same number of electron shells.

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10
Q

How does atomic size increase?

A

Atomic size increases due to an increased number of outer electron shells.

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11
Q

What is the first ionisation energy?

A

The first ionisation energy is the energy that is required to remove a mole of electrons from a mole of gaseous atoms.

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12
Q

What is an endothermic process?

A

An endothermic process is one that takes in energy from it surroundings.

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13
Q

What kind of chemical process is the first ionisation a part of?

A

The endothermic process.

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14
Q

What is the second ionisation energy?

A

The second ionisation energy is the energy that is required to remove one more ion from an element after it already underwent ionisation.

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15
Q

How in the period does the atomic size change?

A

Atomic size decreases going across the period.

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16
Q

Why does the first ionisation energy increase?

A

Due to a decrease in atomic size and an increase in nuclear charge.

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17
Q

Why is it harder to remove an electron that is close to the nucleus?

A

It is closer meaning there is more attraction.

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18
Q

What is the shielding/screening effect of inner electrons?

A

It is the decrease in attraction between an electron and the nucleus in any atom.

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19
Q

Why does the first ionisation energy decrease?

A

It decreases due to the shielding effect of inner electrons and an increase in atomic size.

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20
Q

What is the electronegativity?

A

Electronegativity is the ability of an atom to attract electrons in the bond towards itself.

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21
Q

Why does electronegativity increase?

A

Due to an increase in nuclear charge and a decrease in atomic size.

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22
Q

Why does electronegativity decrease?

A

Electronegativity decreases due to the increasing atomic size and the shielding effect of inner electrons.

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23
Q

What is nuclear charge?

A

Nuclear charge is the total charge of all protons in the nucleus.

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24
Q

What elements have a covalent network bonding?

A

Potassium, Calcium, Aluminium, Magnesium, Sodium, Beryllium, Lithium, Boron, Carbon, Silicon

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25
Q

What elements have a Covalent Small Molecule bonding?

A

Phosphorus, Sulphur

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26
Q

What elements have a Covalent Diatomic bonding?

A

Hydrogen, Nitrogen, Oxygen, Fluorine, Iodine, Chlorine

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27
Q

What elements have a Monatomic bonding?

A

Helium, Neon, Argon

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28
Q

Why do metals conduct electricity?

A

This is because the electrons within the metal are free to move meaning metals can conduct electricity when solid or liquid.

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29
Q

Why do solid metals have high melting and boiling points?

A

This is due to the closely packed lattice structure that contains a lot of bonds that would need to be broken.

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30
Q

How do the metallic bonds become stronger?

A

The more electrons in the outer shell the stronger the metallic bond strength which means that the strength would be increasing across the period due to the increased number of outer shells.

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31
Q

Why would metallic bonding decrease?

A

The strength would decrease down group 1 due to the outer electrons being further from the nuclear charge.

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32
Q

Describe the force of attraction in metallic bonding.

A

It is the electrostatic force of attraction between a ‘sea’ of negatively charged electrons and positively charged metal ions.

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33
Q

What is the sea of electrons called in metallic bonding?

A

Delocalised.

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34
Q

What other things except diatomic metals have covalent molecular bonding?

A

Fullerenes (different forms of carbon)

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35
Q

What are the forces in Covalent Molecular bonds?

A

The intramolecular forces that are within the molecules are all strong covalent bonds, and the intermolecular forces are the bonds between the molecules which are weak London dispersion forces.

36
Q

What increases as more London Dispersion Forces are present?

A

The boiling point.

37
Q

Why does the boiling point of Covalent Molecular structures increase going down the group?

A

The strength of the London Dispersion Forces increases going down the group also meaning that the boiling points increase.

38
Q

What strong intramolecular forces are Covalent Networks linked by?

A

Strong Covalent Bonds.

39
Q

Why do elements with Covalent Network structure have high melting and boiling points?

A

This is because a lot of energy is required to break the strong covalent bonds.

40
Q

What 2 Covalent Network structures does carbon have?

A

Diamond and Graphite.

41
Q

Why don’t elements with Monatomic bonding not bond to other atoms?

A

This is because the elements with Monatomic bonding are all noble gases meaning they have full outer electron shells.

42
Q

What do Monatomic elements exist as?

A

They exist as single atoms.

43
Q

Why do Monatomic Elements not conduct electricity?

A

There are no free electrons.

44
Q

What are the forces between atoms called?

A

Intermolecular Forces.

45
Q

What are the intermolecular forces found in Monatomic elements?

A

London Dispersion Forces.

46
Q

What causes London Dispersion Forces?

A

London Dispersion Forces are caused by an uneven distribution of electrons within an atom. Resulting in a slightly negative and a slightly positive charge on either side of the atom. This is called a temporary dipole.

47
Q

What effect do larger atoms have on the length of temporary dipoles?

A

Larger atoms have more electrons meaning longer dipoles are established.

48
Q

What 2 things do London Dispersion Forces mainly affect?

A

Boiling Point and Melting Point.

49
Q

How are the positive ions in metallic bonding obtained?

A

When metallic bonding happens a metal gives away its outer electron which is then converted to a positive ion.

50
Q

How does Covalent Bonding work?

A

Just like metal bonding it is an electrostatic force of attraction with the atoms being held by the mutual attraction between the positively charged nuclei and the negatively charged electrons.

51
Q

Why do atoms in covalent bonding have the same electronegativity?

A

The atoms within the element are identical.

52
Q

What are London Dispersion Forces?

A

They are a very weak form of bonding between particles which is related to the number of electrons within the atom or molecule meaning bigger particles mean more attraction.

53
Q

Why do noble gases not form any ionic or covalent bonds?

A

They have a full outer electron shell meaning they are stable.

54
Q

What determines the type of bonding in an element?

A

The electronegativity.

55
Q

What are the general rules for electronegativity in relation to bonding?

A

Less than 0.5 means the bond is non-polar covalent, 0.5 to 1.6 means the bond is polar covalent, 1.6 to 2.0 means it is either polar covalent or if a metal and a non-metal are involved it’s ionic, Greater than 2.0 means it is ionic.

56
Q

What is Ionic Bonding?

A

It is an electrostatic force of attraction between positive and a negative ions between metals and non-metals. This creates very strong bonds.

57
Q

What do ionic compounds form instead of molecules?

A

The oppositely charged ions come together to form a large rigid 3 dimensional structure called a lattice.

58
Q

What 2 Covalent compounds exist as a covalent network?

A

Silicon Carbide and Silicon Dioxide.

59
Q

How is polar covalent bonding formed?

A

A polar covalent bond is formed when the attraction of the atoms for the pair of bonding electrons is different.

60
Q

What are the Delta Negative and the Delta Positive Notations used to indicate?

A

They are used to indicate the partial charges on atoms which give rise to a dipole.

61
Q

What does it mean if a molecule is linear?

A

It’s charges are non-symmetrical meaning the molecule is polar.

62
Q

What is said about molecules that contain polar bonds and are non-symmetrical?

A

They have a permanent dipole.

63
Q

What will compounds with polar bonds form?

A

They will form polar molecules if the molecule is not symmetrical.

64
Q

Why are non-polar covalent bonds formed?

A

They are formed when the electrons are shared equally between the atoms.

65
Q

What are intermolecular forces acting between molecules known as?

A

Van Der Waals Forces.

66
Q

What are the main intermolecular force between non-polar molecules?

A

London Dispersion Forces.

67
Q

What are the 3 types of intermolecular forces?

A

London Dispersion Forces, Permanent-Dipole Permanent-Dipole interactions and Hydrogen Bonding.

68
Q

What are Permanent-Dipole Permanent-Dipole interactions?

A

PDP-PDP interactions are an additional electrostatic force of attraction between polar molecules.

69
Q

What intermolecular force is just above LDF in strength?

A

PDP-PDP

70
Q

Where does Hydrogen Bonding exist?

A

In molecules that where a hydrogen atom is attracted to a highly electronegative atom.

71
Q

What is Hydrogen Bonding?

A

Hydrogen Bonding is the electrostatic force of attraction between molecules that contain highly polar bonds.

72
Q

What is the 2nd strongest intermolecular force?

A

Hydrogen Bonding.

73
Q

What is Hydrogen bonding responsible for in water?

A

It is responsible for water being a liquid at room temperature.

74
Q

What properties are related to intermolecular bonding?

A

Melting points, Boiling points, Viscosity, Solubility and Miscibility.

75
Q

What happens to polar molecules if they are put next to a charged rod?

A

They are attracted to it.

76
Q

What are the anomalous boiling points of ammonia, water and hydrogen fluoride the result of?

A

Hydrogen Bonding.

77
Q

Why are the melting and boiling points of polar substances higher than the melting and boiling points of non-polar substances with a similar number of electrons?

A

This is due to the fact that polar substances have PDP-PDP interactions which are stronger than the LDF found in non-polar substances.

78
Q

What should you do when comparing intermolecular bonding?

A

Choose molecules of similar mass as that would mean that any differences that there are are not due to different LDF.

79
Q

What is Viscosity related to?

A

The strength of the intermolecular forces that exist between the molecules.

80
Q

What does a higher number of hydrogen bonds do in a liquid?

A

Make it more viscous.

81
Q

What molecules to do polar molecules dissolve with?

A

Polar molecules (like dissolves like)

82
Q

What molecules do non-polar molecules dissolve with?

A

Non-polar molecules (like dissolves like)

83
Q

What is the result of water being attracted to the oppositely charged ions in the ionic lattice?

A

It breaks the ionic lattice apart.

84
Q

What does hydrogen bonding in ice result in?

A

It results in an expanded structure that causes the density of ice to be less than that of water at low temperatures.

85
Q

Why does ice float on water?

A

This is due to ice being less dense than water as hydrogen bonding within it forces the molecules into an open lattice structure as it reaches its freezing point.

86
Q

What happens to water between 0 and 4 Degrees Celsius?

A

The water expands again as the molecules are rearranged into in a rigid crystal lattice structure.

Higher Chemistry (3 decks)

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