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chemical bonding Flashcards

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1
Q

definition of element

A

contains only 1 kind of atoms, cannot be broken down into simpler substances

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2
Q

define compound

A

2 or more atoms of different elements, chemically bonded together

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3
Q

define mixture

A

mixture contains different substances that are not bonded tgt

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4
Q

what are the 3 signs of chemical change

A

1) one or more new chemical substances are formed
2) energy is take in or given out
3) change is difficult to reverse

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5
Q

define physical change

A

when no new chemical substance is formed

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6
Q

in molecules and compounds, atoms are held tgt by _____

A

chemical bonds

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7
Q

why do atoms form bonds?

A

to gain a stable arrangement of outer shell electrons, like grp 8
makes them more chemically stable

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8
Q

what is valency

A

number of electrons an atoms uses for bonding

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9
Q

how many valency does iron(III) have

A

3 i think

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10
Q

what is ionic bonding?

A

the strong electrostatic force of attraction between oppositely- charge ions/ bond that forms between ions of opposite charge

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11
Q

do metal or non metals form an anion during ionic bonding?

A

non metals

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12
Q

true or false: the charge of ion does not reflect the number of electrons it has gained or lost.

A

false

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13
Q

what is group’s 1 ionic charge?

A

+1

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14
Q

what is groups 2 ionic charge

A

+2

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15
Q

true or false: the charge of ions does reflect the number of electrons it has gained or lost ?

A

true

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16
Q

what is group 3 ionic charge?

A

+3

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17
Q

what is the ionic charge for grp 7,6,5

A

-1,-2,-3

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18
Q

what is the pattern that is formed in ionic bond

A

lattice , alternating positive and negative ions

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19
Q

what are the 4 properties of ionic compounds

A

high m&b points, hard and brittle, soluble in water but insoluble in organic solvent , can conduct electricity in aqueous but not solid

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20
Q

does ionic compound have high or low melting points? why

A

high; strong EFOA holds the oppositely charged ions tgt in the lattice.
because the ionic bond is very strong, it takes a lot of heat to overcome these strong forces

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21
Q

can the ionic compounds conduct electricity? why or why not

A

solid cannot conduct electricity because in solid state, ions are vibrating at fixed position and do not move freely. but when it melts or dissolves in water to form a solution it can because the ions are moving freely. since the ions are charges, they can carry electrical charges and conduct electricity

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22
Q

is ionic compounds soluble in water? why or why not?

A

it is soluble in water because water molecules are able to separates the ions from each other. when the ions move apart, they will be surrounded by water molecules

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23
Q

does hydrogen lose or gain electrons

A

lose electrons to from positive ion

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24
Q

why do they element in grp 4 and 5 not form ions?

A

they wld hv to gain or lose several electrons and that’s takes up too much energy

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25
Q

why do grp 8 not form ions?

A

because they already have a stable outer shell, so they do not need to gain or loses electrons

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26
Q

true or false: some metals can form more than one type of ion.

A

true

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27
Q

what transitional metal forms more than 1 type of ion and which don’t

A

copper and iron ; zinc and silver

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28
Q

what are compound ions?

A

ions that are formed from a group of bonded atoms

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29
Q

what is a giant ionic structure

A

when ions are arranged in geometric 3D patterns which go one forever

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30
Q

true or false: all ionic compound do not have giant ionic structure

A

false

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31
Q

what is a crystalline structure

A

the regular arrangement of ions in the lattice

32
Q

are ionic crystals brittle? why

A

yes, because once layer of ions in the crystals has been forced to move, ions of the same charge will be next to each other and will repel, splitting the crystal

33
Q

what is metallic bond

A

strong EFOA between the metals cations and negative ‘sea’ of electrons tgt in a lattice

34
Q

why does metal atoms get packed tightly tgt in a regular lattice?

A

to allow outer electrons separate from their atoms. results is a lattice of ions on a ‘sea’ of electrons that are free to move

35
Q

what does the regular arrangement of ions results in?

A

crystals

36
Q

physical properties of a metal?

A

high melting and boiling pints, conduct h&e, malleable and ductile and hard

37
Q

why does metal conduct heat in solid and liquid

A

free electrons take in heat energy
move faster
quickly transfer heat though metal structure

38
Q

why can metal conduct electricity

A

delocalized (removed) electrons move freely though the metal lattice to carry electrical charges
free electrons can move through the lattice carrying charge

39
Q

why do metal have high melting and boiling point?

A

strong EFOC between metal cations and negative sea of electrons
lot of heat needed to overcome the force of attraction

40
Q

why are metal malleable and ductile

A

cation layer can slides past each other without breaking when force is applied
layers can slides without breaking metallic bond because electrons are free to move

41
Q

why are metals hard

A

strong EFOA between metal cation and negative sea of electrons
a lot of force needed to overcome these metallic bond

42
Q

what is the structure of metallic bond

A

layers of positively charged metal ions in the sea of electron in a lattice

43
Q

what is covalent bond

A

non-metal atoms form bonds with other non-metals by sharing pairs of electrons
EFOA between nuclei of atoms combining with the shared electrons

44
Q

why do non metal atoms not give up electrons to gain a full outer shell?

A

they would have to lose too many which wld take up too much energy to overcome the pull of positive nucleus

45
Q

true or false: when 2 non-metals react tgt, only one of them needs to gain enough electron to achieve a stable outer shell.

A

false

46
Q

what is single, double and triple covalent bond and their short forms

A

a covalent bond when a pair of electrons is shared between 2 atoms cl-cl
a covalent bond when 2 pairs of electrons are shared between 2 atoms0=0
a covalent bonds when 3 pairs of electrons are shared between 2 atoms N≡N

47
Q

what is simple molecular structure

A

substances with covalent bonding that made of molecules

48
Q

properties of simple covalent molecules

A

soluble in organic solvent, insoluble in water, low m&e points, cannot conduct electricity, soft and brittle

49
Q

why do simple covalent molecules have low/ high melting points

A

low; covalent bond between atoms in a molecule is strong but the force of attraction between the molecules ( intermolecular force) is very weak
less heat needed to overcome these weak forces between molecules
**only intermolecular force is broken not the covalent bonds between atoms

50
Q

why is covalent molecules poor or good heat and electrical conductors

A

consist of only simple molecules and has no free moving ions/ electrons present

51
Q

what are covalent compounds?

A

atoms of different elements share electrons

52
Q

what dictates the shape of molecules?

A

pairs of electrons ard atoms repel each other
move as far part as they can
gives a tetrahedral shape or linear shape

53
Q

why do water molecules appear to be bent

A

4 electrons pair ard oxygen

take up tetrahedral shape

54
Q

similarities of covalent and ionic

A

both hv regular lattice in solid state and form crystals

55
Q

2 differences between ionic and covalent in terms of forces

A

ionic solids particles are charged and forces are strong

molecular covalent solids particles are not charged and forces between them are weak

56
Q

difference in properties of ionic and covalent compounds

A

ionic hv high m&b points, soluble in water and can conduct electricity when melted or dissolved in water
covalent molecules hv low m&b points, insoluble in water and do not conduct electricity

57
Q

what solvent can covalent compounds dissolve in?

A

tetrachloromethane

58
Q

what are giant covalent molecules

A

atoms are bonded by strong covalent bonding in a giant structure
not hold tgt by weak lattices
exist in giant covalent structure or macromolecules

59
Q

what are some examples of giant covalent molecules

A

graphite, diamond and silicon

60
Q

what are allotropes? what are allotropes of carbon

A

2 forms of the same element; graphite and diamond

61
Q

properties of giant covalent molecules

A

giant covalent lattice, high m&e points, no electrical conductivity for solids, solutions or liquid, very hard

62
Q

structure of diamond

A

each carbon atoms is covalently bonded to 4 other carbon atoms, arranged tetrahedrally in a giant structure

63
Q

physical properties of diamond

A

hard, do not conduct electricity and high m&e points

64
Q

do diamonds conduct electricity? why or why not

A

does not conduct; no mobile electrons as all carbon atoms have used their valence electron for bonding

65
Q

why is diamond a hard material

A

strong covalent bonds joining atoms tgt in a tetrahedron structure
a lot of force needed to overcome the bond

66
Q

why does diamond have low/ high melting and boiling points

A

a lot of energy needed to break the strong covalent bond that joins carbon atoms tgt in a giant structure

67
Q

uses of diamond

A

cut edges of drills or saws because diamond is hard it good to cut edges of saw as it must cut through hard materials such as metals or ceramics
jewellery

68
Q

graphite structure

A

each carbon atoms is bonded with 3 other carbon atoms in hexagonal carbon rings in layers

69
Q

physical properties of graphite

A

conduct electricity, soft, high m&b points

70
Q

why does graphite conduct/ not conduct electricity

A

conducts electricity because other shell electrons from each carbon atom is delocalised between layers
carbon atom has 4 outer electrons but only forms 3 bonds
forth electrons is free to move though graphite, carrying charge

71
Q

why is graphite hard/ soft

A

soft

layers are attracted by weak intermolecular forces so layers easily slides over each other when force is applied

72
Q

why does graphite hv high or low m&b points

A

high because covalent bond joining carbon atoms in layers are very strong
a lot of heat needed to overcome the bond

73
Q

uses of graphite

A

electrical conductor (insert, conducts e, high m point)
lead
lubricant for engines and locks

74
Q

structure of silicon dioxide

A

each silicon atoms is covalently bonded to 4 oxygen atoms and each oxygen atoms is covalently bonded to 2 silicon atoms, arranged tetrahedrally in a giant structure

75
Q

physical properties of silicon dioxide and why?

A

hard, does not conduct electricity, high m&b points , same reasons as diamonds

chemistry (9 decks)

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