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Chemisty > Chemical Bonding > Flashcards

Chemical Bonding Flashcards

1
Q

what is chemical bonding?

A

attraction between atoms involving electron transfer/sharing to form new compounds

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2
Q

what is a grouped ion?

A

more than one atom involved in the ion

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3
Q

what is the symbol for carbonate and its charge?

A

symbol = CO3

charge = 2-

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4
Q

what is the symbol for ammonium and its charge?

A

symbol = NH4

charge = 1+

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5
Q

what is the symbol and charge for hydroxide?

A

symbol = OH

charge = 1-

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6
Q

what is the symbol and charge for nitrate?

A

symbol = NO3

charge = 1-

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7
Q

what is the symbol and charge for sulfate?

A

symbol = SO4

charge = 2-

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8
Q

what is the symbol and charge for phosphate?

A

symbol = PO4

charge = 3-

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9
Q

what is valency?

A

the number of electrons an atom needs to complete the outer shell

those electrons are either gained or lost

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10
Q

do non-metals gain or lose electrons?

A

gain

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11
Q

what is an ion

A

a charged particle (positive or negative)

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12
Q

how does the cross rule work?

A
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13
Q

are metals negatively or positively charged and why?

A

positively charged (cations)

they lose electrons

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14
Q

are non-metals negatively or positively charged and why?

A

negatibely charged (anions)

they gain electrons

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15
Q

in the centre of the atom are two sub-atomic particles

these particles are the …… and the …..

the ….. are positively charges

the ……have no charge and are …..

A

in the centre of the atom are two sub-atomic particles

these particles are the protons and the neutrons

the protons are positively charged

the **neutrons **have no charge and are neutral

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16
Q

the centre of an atom is ….. charged

A

the centre of an atom is positively charged

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17
Q

around the centre of the atom are negatively charges sub-atomic particles called …..

A

around the centre of the atom are negatively charges sub-atomic particles called electrons

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18
Q

the overall charge on an atom is ….

the number of …… and …… are equal

A

the overall charge on an atom is zero

the number of **protons and electrons **are equal

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19
Q

electrons are arranged in energy …. around the centre of the atom

the first energy …. is nearest to the centre and can take a maximum of …. electrons

the second and thur energy …. can take a maximum if …. electrons each

A

electrons are arranged in energy **shells **around the centre of the atom

the first energy shell is nearest to the centre and can take a maximum of 2 electrons

the second and thur energy shells can take a maximum if 8 electrons each

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20
Q

when atoms bond with other atoms, the number of electrons in their outermost energy shell ……

A

when atoms bond with other atoms, the number of electrons in their outermost energy shell changes

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21
Q

what are elements

A

substances that can’t be split into anything more simply by chemical means

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22
Q

what do all atoms in elements share?

A

the same atomic number

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23
Q

how are elements recognised in diagram?

A

the atoms have the same size or colour

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24
Q

what are compounds?

A

a combination of two or more elements in fixed proportions, joined together by strong bonds

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25
Q

does it matter if the compound is molecular, giant covalent or giant ionic?

A

no

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26
Q

what is a mixture?

A

the various components can be in any proportions

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27
Q

is an alloy a mixture? why?

A

yes because of the totally variable proportions

28
Q

what is the differences in proportions between mixtures and compounds

A

A compounds proportions never vary

In a mixture the portions vary

If you wanted to mix some silvery zinc metal with some yellow sulphur, you could use any proportions

in zinc sulphide the proportions of zinc and sulphur have to be the exact same

29
Q

what is the differences in properties between mixtures and compounds

A

in elements, each element has its own properties, but the properties of the compound are different

a mixture of hydrogen and oxygen would explode when you put it in a flame

a compound of hydrogen and oxygen to make water would put out a flame

30
Q

what is the differences in ease of separation between mixtures and compounds

A

mixture can be separated by physical means

e.g. change in temperature, or dissolving part of the mixture in a solvent like water, things that do not involve chemical reactions

compounds have to be separated by chemical reactions

e.g. electrolysis

31
Q

what is the differences in energy change between mixtures and compounds

A

there is little to no energy changes when making a mixture

there is greater energy changes when making a compound

32
Q

explain why hydrogen is gas at room temperature

A

hydrogen is a simple molecule and so has weak intermolecular forces between its molecules

these weak forces break at room temperature

33
Q

hydrogen chloride has a …… molecular structure

there are …. forces between the ….

because of this, hydrogen chloride has a ….. boiling point

A

hydrogen chloride has a simple molecular structure

there are weak forces between the molecules

because of this, hydrogen chloride has a low boiling point

34
Q

why is pure copper malleable?

A

pure metals are malleable because of their same sized atoms and arrangement

layers can easily slide over each other because in metals there are delocalised electrons which allow copper ions to do this

35
Q

bronze is a mixture of tin and copper, the tin atoms are much bigger than the copper atoms

why is bronze not as malleable as copper

A

the different size of atoms (tin is much bigger than copper) mean that they can’t slide over each other

36
Q

why do metals conduct electricity?

A

delocalised electrons fall between the layer of atoms and conduct electricity

37
Q

a substance has:

melting point = 540C

boiling point = 1200C

electrical conductivity as solid = poor

electrical conductivity as liquid = poor

electrical conductivity as aqueos solution = poor

what type of structure is it?

A

covalent: simple

38
Q

a substance has:

melting point = 4030C

boiling point = 5670C

electrical conductivity as solid = good

electrical conductivity as liquid = good

electrical conductivity as aqueos solution = not soluble

what type of structure is it?

A

metallic

39
Q

a substance has:

melting point = -2100C

boiling point = -1960C

electrical conductivity as solid = poor

electrical conductivity as liquid = poor

electrical conductivity as aqueos solution = poor

what type of structure is it?

A

covalent: simple

CHECK

40
Q

a substance has:

melting point = 16100C

boiling point = 22300C

electrical conductivity as solid = poor

electrical conductivity as liquid = poor

electrical conductivity as aqueos solution = not soluble

what type of structure is it?

A

covalent: giant

41
Q

a substance has:

melting point = 6150C

boiling point = 8760C

electrical conductivity as solid = poor

electrical conductivity as liquid = good

electrical conductivity as aqueos solution = good

what type of structure is it?

A

ionic

42
Q

a substance has:

melting point = 37270C

boiling point = 48270C

electrical conductivity as solid = good

electrical conductivity as liquid = good

electrical conductivity as aqueos solution = not soluble

what type of structure is it?

A

metallic

43
Q

a substance has:

melting point = 560C

boiling point = 3420C

electrical conductivity as solid = good

electrical conductivity as liquid = good

electrical conductivity as aqueos solution = good

what type of structure is it?

A

metallic

44
Q

a substance has:

melting point = 9340C

boiling point = 15680C

electrical conductivity as solid = poor

electrical conductivity as liquid = good

electrical conductivity as aqueos solution = insoluble

what type of structure is it?

A

ionic

45
Q

a substance has:

melting point = -1050C

boiling point = -450C

electrical conductivity as solid = poor

electrical conductivity as liquid = poor

electrical conductivity as aqueos solution = good

what type of structure is it?

A

covalent: simple

CHECK

46
Q

state whether you would expect calcium flouride (ionic bonding) to have a high or low melting point and why

A

high

stronger attraction between the positive Cl atoms and negative F atoms

lots of energy needed

47
Q

what is the chemical formula for Calcium Flouride

A

CaF2

48
Q

what is the chemical formula for Potassium Bromide

A

KBr

49
Q

what is the chemical formula for Barium NItrate

A

Ba(NO3)2

50
Q

what is the chemical formula for Beryllium Oxide

A

BeO

51
Q

what is the chemical formula for magnesium phosphate

A

Mg3(PO4)2

52
Q

what does the ‘(II)’ in Copper (II) indicate?

A

each copper atom contributes 2 electrons

53
Q

why can copper conduct electricity?

A

because it has a sea of delocalised electronsnbetween the layers in the structure which are free to move

54
Q

why can copper be drawn into wires

A

copper is ductile

the sea of delocalise delectrons mean the layers can slide easily over each other and be drawn into wires

55
Q

what is a use for poly(ethene)

A

wax in polish

56
Q

why does propanone and water (both simple molecular structures) have low boiling points

A

the attractive forces between their molecules are weak

these require little energy to be overcome

57
Q

ammonia is:
ionic bonding / covalent bonding

insoluble in water / soluble in water

A

covalent bonding

soluble in water

58
Q

methane is:
ionic bonding / covalent bonding

insoluble in water / soluble in water

A

covalent bonding

insoluble in water

59
Q

poly(ethene) is:
ionic bonding / covalent bonding

insoluble in water / soluble in water

A

covalent bonding

insoluble in water

60
Q

sodium chloride is:
ionic bonding / covalent bonding

insoluble in water / soluble in water

A

check

61
Q

sodium hydroxide is:
ionic bonding / covalent bonding

insoluble in water / soluble in water

A

ionic bonding

soluble in water

62
Q

give two observations made during the reaction between magnesium and oxygen

A

a huge bright light is seen

a sizzle is heard whilst the reaction occurs

63
Q

why is the melting point of magnesium oxide much higher than that of sodium chloride?

A

lattice is held together by stronger attraction

this is because the ions have a higher charge and therefore a higher attraction

64
Q

Suggest and explain why silica is used to make bricks for high-temperature furnaces. In your answer, you should refer to the structure of, and bonding im, silica

A

giant covalent stucture

strong covalent bonds between atoms

lots of energy to breka bonds - makes them suitable to withdstand heat

65
Q

When glue sets it forms a giant covalent structure

explain why the giant covalent structures have high melting points?

A

they have strong covalent bonds which take a lot of energy to break so it needs to be a high heat to break these bonds

Chemisty (20 decks)

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