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chemical bonding Flashcards

(75 cards)

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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
why do grp 8 not form ions?
because they already have a stable outer shell, so they do not need to gain or loses electrons
26
true or false: some metals can form more than one type of ion.
true
27
what transitional metal forms more than 1 type of ion and which don't
copper and iron ; zinc and silver
28
what are compound ions?
ions that are formed from a group of bonded atoms
29
what is a giant ionic structure
when ions are arranged in geometric 3D patterns which go one forever
30
true or false: all ionic compound do not have giant ionic structure
false
31
what is a crystalline structure
the regular arrangement of ions in the lattice
32
are ionic crystals brittle? why
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
what is metallic bond
strong EFOA between the metals cations and negative 'sea' of electrons tgt in a lattice
34
why does metal atoms get packed tightly tgt in a regular lattice?
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
what does the regular arrangement of ions results in?
crystals
36
physical properties of a metal?
high melting and boiling pints, conduct h&e, malleable and ductile and hard
37
why does metal conduct heat in solid and liquid
free electrons take in heat energy move faster quickly transfer heat though metal structure
38
why can metal conduct electricity
delocalized (removed) electrons move freely though the metal lattice to carry electrical charges free electrons can move through the lattice carrying charge
39
why do metal have high melting and boiling point?
strong EFOC between metal cations and negative sea of electrons lot of heat needed to overcome the force of attraction
40
why are metal malleable and ductile
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
why are metals hard
strong EFOA between metal cation and negative sea of electrons a lot of force needed to overcome these metallic bond
42
what is the structure of metallic bond
layers of positively charged metal ions in the sea of electron in a lattice
43
what is covalent bond
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
why do non metal atoms not give up electrons to gain a full outer shell?
they would have to lose too many which wld take up too much energy to overcome the pull of positive nucleus
45
true or false: when 2 non-metals react tgt, only one of them needs to gain enough electron to achieve a stable outer shell.
false
46
what is single, double and triple covalent bond and their short forms
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
what is simple molecular structure
substances with covalent bonding that made of molecules
48
properties of simple covalent molecules
soluble in organic solvent, insoluble in water, low m&e points, cannot conduct electricity, soft and brittle
49
why do simple covalent molecules have low/ high melting points
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
why is covalent molecules poor or good heat and electrical conductors
consist of only simple molecules and has no free moving ions/ electrons present
51
what are covalent compounds?
atoms of different elements share electrons
52
what dictates the shape of molecules?
pairs of electrons ard atoms repel each other move as far part as they can gives a tetrahedral shape or linear shape
53
why do water molecules appear to be bent
4 electrons pair ard oxygen | take up tetrahedral shape
54
similarities of covalent and ionic
both hv regular lattice in solid state and form crystals
55
2 differences between ionic and covalent in terms of forces
ionic solids particles are charged and forces are strong | molecular covalent solids particles are not charged and forces between them are weak
56
difference in properties of ionic and covalent compounds
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
what solvent can covalent compounds dissolve in?
tetrachloromethane
58
what are giant covalent molecules
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
what are some examples of giant covalent molecules
graphite, diamond and silicon
60
what are allotropes? what are allotropes of carbon
2 forms of the same element; graphite and diamond
61
properties of giant covalent molecules
giant covalent lattice, high m&e points, no electrical conductivity for solids, solutions or liquid, very hard
62
structure of diamond
each carbon atoms is covalently bonded to 4 other carbon atoms, arranged tetrahedrally in a giant structure
63
physical properties of diamond
hard, do not conduct electricity and high m&e points
64
do diamonds conduct electricity? why or why not
does not conduct; no mobile electrons as all carbon atoms have used their valence electron for bonding
65
why is diamond a hard material
strong covalent bonds joining atoms tgt in a tetrahedron structure a lot of force needed to overcome the bond
66
why does diamond have low/ high melting and boiling points
a lot of energy needed to break the strong covalent bond that joins carbon atoms tgt in a giant structure
67
uses of diamond
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
graphite structure
each carbon atoms is bonded with 3 other carbon atoms in hexagonal carbon rings in layers
69
physical properties of graphite
conduct electricity, soft, high m&b points
70
why does graphite conduct/ not conduct electricity
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
why is graphite hard/ soft
soft | layers are attracted by weak intermolecular forces so layers easily slides over each other when force is applied
72
why does graphite hv high or low m&b points
high because covalent bond joining carbon atoms in layers are very strong a lot of heat needed to overcome the bond
73
uses of graphite
electrical conductor (insert, conducts e, high m point) lead lubricant for engines and locks
74
structure of silicon dioxide
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
physical properties of silicon dioxide and why?
hard, does not conduct electricity, high m&b points , same reasons as diamonds

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