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chemistry > booklet 2-bonding > Flashcards

booklet 2-bonding Flashcards

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1
Q

when are bonds formed

A

when atoms react

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2
Q

what are bonds

A

“glue” that holds atoms together

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3
Q

what are three things that can happen to electrons in bonding

A

lost gained or shared

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4
Q

what are the three types of bonding

A

ionic covalent and metalic

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5
Q

what sort of atoms does ionic bonding take place with

A

metals and non metals

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6
Q

what happens to electrons in ionic bonding

A

they are lost or gained +or-

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7
Q

how do metals behave im ionic bonding

A

they loose their outer electrons to become positive ions and have a full outer shell

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8
Q

what happens when an alkali metal like sodium reacts

-what charge and why

A

it looses its outer electron to have a +1 charge as it now has one more proton than electron

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9
Q

what do we call this charged atom (sodium in this case)

A

an ion - positive sodium ion

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10
Q

how do none metals behave

A

they gain the outer electrons off the metals to gain full outer shells and become-1 charge negatively charged ions

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11
Q

what happens when a halogen like chlorine reacts

A

group 7 element gains one outter electron

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12
Q

what is the charge of a chloRIDE ion

A

-1

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13
Q

what does it have the same electron configuration as

A

a noble gas

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14
Q

where do metals loose their outer electron to

A

non metals

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15
Q

why are they happy to gain the electron

A

to gain a full outer shell

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16
Q

what do they both now have

A

full outer shells

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17
Q

what ions do metals form

A

positive +1

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18
Q

what ions do non metals form

A

negative-1

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19
Q

these oppositely charged ions what

A

attract

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20
Q

by what forces do they attract

A

electrostatic attraction forces

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21
Q

what are the valencies of a metal

A

the same as the group number

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22
Q

what are the valencies in a non metal

A

8 minus the group number

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23
Q

valency is the same as what

A

valency is the same as the charge of an atom

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24
Q

ionic compounds are formed between what

A

metals and non metals

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25
Q

positive and negative ions form what

A

ionic bonds

26
Q

what do these ionic bonds between positive and negative ions form

A

a giant ionic lattice

27
Q

electrostatic forces of attraction are acting in what

A

all six directions-3dimensons

28
Q

how strong are the electrostatic forces of attraction

A

they are strong

29
Q

what does it give the compound

A

high melting and boiling points

30
Q

ionic compounds conduct what

A

electricity

31
Q

when do they conduct this

A

when molten or dissolved in water

32
Q

why will they conduct this

A

because electrostatic forces are broken and charged ions are free to move and carry current

33
Q

when will they not conduct

A

ionic compounds will not conduct electricity when solid as ions cannot move so cannot carry current

34
Q

what sort of elements does covalent bonding take place in

A

non metal and non metal

35
Q

what are non metals short of

A

non metals are short of electrons in their outer shell and they require full shells to be happy

36
Q

what do they do with electrons if a metal is not present to give an electron

A

they share electrons in pairs with another non metal

37
Q

what is made when the electrons are shared

A

a covalent bond is made

38
Q

what is to be remembered about covalent bonds

A

covalent bonds are STRONG

39
Q

what to ways can yu show covalent bonds

A

dot and cross form

stick form

40
Q

what elements does metallic bonding take place in

A

metals and metals

41
Q

what do metals conduct

A

heat and electricity

42
Q

why do metals conduct heat and electricity

A

because their electrons in their outer shells are free to move and carry current

43
Q

what do metals form structure wise

A

a giant lattice of positive ions in a sea of delocalised electrons that are negative

44
Q

what do the electrons do in metallic bonding

A

they are free to move enabling heat and electricity to be conducted this movement also meants they attract deattract and reattract to each atom as they move about

45
Q

what holds the atoms

A

forces of electrostatic attraction

46
Q

what structure to the forces of electrostatic attraction hold the atoms in

A

in a regular structure

47
Q

what are the forces like

A

very strong and hard to break

48
Q

what do strong forces of electrostatic attraction result in

A

high melting points and hight boiling points

49
Q

what does the regular structure of the metals result in

A

the layers of atoms can slide over eachother and metals can be bent and shaped they are malleable

50
Q

what are alloys

A

alloys are mixtures made from two different metals

51
Q

what happens when you add different size metals

A

different size metals distort the regular structure of pure metal and the layers cannot slide

52
Q

what are alloys conpared to pure metals

A

alloys are harder than pure metals

53
Q

what are the bonds like between solids particles

A

strong bonds

54
Q

what do solids require a lot of to change and what to

A

solids require a large about of heat energy to melt from a solid to a liquid so it has a high melting point

55
Q

what happens if the bonds in liquid particles are strong

A

they will require a large amount of heat energy to boil or evaporate the liquid to a gas

56
Q

what two things does the strength of bonds depend upon

A

1- nature of thr particle

2-type of bonding holding together particles

57
Q

ionic compounds only contain what with what

A

strong ionic bonds which have a high melting point

58
Q

giant covalent structures contain only what and boiling point

A

covalent bonds with high melting point

59
Q

some covalent structures also have what

A

weak forces of attraction between molecules

60
Q

what are these forces also called

A

intermolecular forces or van der waals

61
Q

what happens to these forces when a covalent structure melts and at what temperature

A

forces break and usually at a low temperature

chemistry (7 decks)

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