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Higher Chemistry > unit 1 > Flashcards

unit 1 Flashcards

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1
Q

metallic elements within the first 20

A

Lithium
Beryllium
Sodium
Magnesium
Aluminium
Potassium
Calcium

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2
Q

covalent molecular elements within the first 20

A

H2
N2
O2
F2
Cl2
P4
S8
carbon in form of fullerene (C60)

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3
Q

covalent network elements within the first 20

A

Boron
Silicon
Carbon (diamond and graphite)

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4
Q

what is meant by the term covalent radius?

A

measure of the size of an atom from the nucleus to the outermost electron shell

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5
Q

covalent radius going across a period

A

decreases

nuclear charge increases

therefore, electrons are pulled closer to the nucleus

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6
Q

covalent radius going down a group

A

increases

more electron shells so increased shielding

therefore electrons have a weaker pull towards the nucleus

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7
Q

what is meant by the first ionisation energy?

A

energy required to remove one mole of electrons from one mole of gaseous atoms

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8
Q

what is meant by the second ionisation energy?

A

energy required to remove the 2nd mole of electrons from one mole of gaseous atoms

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9
Q

ionisation energy going across a period

A

increases

nuclear charge increases

pull on outer electrons is stronger so it is harder to remove them

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10
Q

ionisation energy going down a group

A

decreases

more electron shells so increased shielding

therefore electrons have a weaker pull towards the nucleus making it easier to remove them

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11
Q

removing electrons from a full outer shell increased ionisation energy

A

involves the removal of an electron from a full electron shell

this electron shell is also strongly pulled towards the nucleus compared to the previous shell

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12
Q

what is meant by the term electronegativity?

A

the strength an atom has for bonded electrons

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13
Q

how to atoms get a delta -/+ charge?

A

in polar molecules

the atom with the stronger electronegativity pulls the electrons closer given them a delta - charge and the other atom a delta + charge

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14
Q

electronegativity going across a period

A

increases

nuclear charge increases causing the atom to be smaller

stronger attraction on outer electrons

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15
Q

electronegativity going down a group

A

decreases

more electron shells so increased shielding

less attraction on outer electrons

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16
Q

why do noble gases not have an electronegativity value?

A

unreactive/cannot form bonds

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17
Q

intramolecular bonding

A

strong bonds between atoms in the same molecule

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18
Q

intermolecular bonds

A

weak bonds between molecules

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19
Q

intermolecular bonds in increasing strength

A

LDF’s
pd-pd interactions
hydrogen bonding

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20
Q

covalent bonding

A

two positive nuvelei being held together by their common attraction for the shared pair of electrons

21
Q

ionic bonding

A

electrostatic attraction between positive and negative ions forming a lattice

22
Q

non-polar covalent bonds

A

forms between atoms with the same electronegativity values

23
Q

polar covalent bonds

A

atoms have different electronegativity values so there is an uneven sharing of electrons

24
Q

what is a dipole?

A

uneven distribution of electrons

25
Q

what type of dipole is found in polar molecules?

A

permanent

26
Q

describe the bonding continuum?

A

electronegativity difference
OR ionic character

least - non-polar
middle - polar
high - ionic

27
Q

how can polar bonds be overall non-polar?

A

bonds are symmetrically opposed and will cancel out

28
Q

intermolecular forces (van der Waals) in order of increasing strength

A

LDF’s
PD-PD interactions
H bonding

29
Q

where do LDF’s occur?

A

between all molecules

30
Q

how are LDF’s formed?

A

forces of attraction between temporary dipoles and induced dipoles in nearby molecules

31
Q

how is the strength of an LDF determined?

A

the more electrons = the stronger it is

32
Q

where do PD-PD interactions occur?

A

in polar molecules

33
Q

where does hydrogen bonding occur?

A

in bonds where hydrogen is bonded to either Nitrogen, Oxygen or Fluorine

34
Q

bonding in monatomic

A

held together by weak LDF’s

35
Q

what bonds break in a covalent network?

A

covalent bonds

36
Q

what bonds are broken in covalent moleculars?

A

the Van Der Waal force

37
Q

why when comparing MP we need similar GFMs?

A

similar LDF strength

38
Q

bonds in order of decreasing strength

A

covalent network
ionic
metallic
polar
non-polar
monatomic

39
Q

explain the structure of ice

A

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

40
Q

how is viscosity measured?

A

as the number of H bonds increases, the viscosity increases

41
Q

what is a reducing agent?

A

substance that donates electrons
thing being oxidised

42
Q

what is an oxidising agent?

A

substance that accepts electrons
thing being reduced

43
Q

low electronegativity
reducing or oxidising agent?

A

from ions by losing electrons so act as reducing agents

44
Q

high electronegativity
reducing or oxidising agent?

A

form ions by gaining electrons and act as oxidising agents

45
Q

where can the strongest reducing agents be found?

A

group 1
top right of the ECS

46
Q

oxidising agent examples

A

hydrogen peroxide
dichromate and permanganate ions in acidic solutions

47
Q

where can the strongest oxidising agents be found?

A

group 7
bottom left of the ECS

48
Q

reducing agent examples

A

carbon monoxide

49
Q

oxidising agent uses

A

kill fungi and bacteria
inactivate viruses
breaking down coloured compounds - bleach

Higher Chemistry (5 decks)

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