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Jr 1 - chem > atomic structure and bonding > Flashcards

atomic structure and bonding Flashcards

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1
Q

define what an atom is

A

the smallest particles of matter that cannot be broken down any further

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2
Q

what particles are in the nucleus

A

protons and neutrons

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3
Q

what is the mass of an atom measured in

A

atomic mass units

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4
Q

which of the three is the lightest particle

A

electrons

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5
Q

mass of protons

A

1 unit

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6
Q

mass of electrons

A

almost nothing

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7
Q

mass of neutrons

A

1 unit

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8
Q

where is the mass number on the symbol of an element

A

on the top

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9
Q

where is the proton number on the symbol of an element

A

on the bottom

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10
Q

how can you identify an atom using protons

A

by the number of protons

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11
Q

another name for proton number

A

atomic number

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12
Q

why do atoms have no charge

A

because they contain the same number of proton and electrons

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13
Q

define mass number

A

to total number of protons and neutrons in an atom

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14
Q

another name for mass number

A

nucleon number

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15
Q

do ions have electronic charge

A

yes

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16
Q

why are ions charged

A

ions gain and lose electrons. when they gain an electron they become negatively charged. when they lose an electron they become positively charged. (the number of protons does not change)

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17
Q

why do atoms form ions

A

because they gain or lose electrons to obtain a stable outermost shell

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18
Q

define ‘isotopes’

A

atoms of the same element that have a different neutron number but same proton number (have different nucleon number)

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19
Q

what are the 2 types of isotopes

A

stable and unstable isotopes

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20
Q

why are some isotopes unstable

A

because the the extra neutrons are radioactive

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21
Q

what are unstable isotopes called

A

radioisotopes

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22
Q

why are radioisotopes radioactive

A

because the nucleus is unstable. the atoms naturally will break down or decay giving out radiation in the form of particles and rays, plus a large amount of energy.

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23
Q

define relative atomic mass

A

the average mass of a large number of atoms of an element

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24
Q

what is the symbol for relative atomic mass

A

Ar

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25
Q

what is the standard used for the Ar scale

A

carbon-12

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26
Q

what is the Ar formula

A

avg. mass of isotopes of an element/ 1/12 x mass of 1 atom of carbon 12

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27
Q

which electron shell has the highest energy level

A

the outermost electron shell

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28
Q

what is another name of the outer- shell electrons

A

valency electrons

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29
Q

why don’t unreactive atoms form bonds

A

because they have a stable arrangement of electrons in their outermost shell which does not allow them to bond with other atoms

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30
Q

why do atoms form bonds

A

to gain a stable outermost electron shell

31
Q

define an ionic bond

A

a chemical bond between a metal and non-metal

32
Q

how do solid ionic compounds formed

A

the form a lattice of alternation positive and negative ions that are held together by strong ionic bonds

33
Q

define ‘lattice’

A

the arrangement of atoms

34
Q

why don’t group 4 and 5 elements use ionic bonds

A

because they have to gain or lose to many electrons and it take too much energy.

35
Q

what are compound ions

A

ions formed from a group of bonded atoms.

36
Q

define covalent bonds

A

a bond where atoms share the electrons in their outer energy levels. this occurs between non-metal atoms.

37
Q

define ‘molecule’

A

a group of atoms held together by covalent bonds.

38
Q

what are elements made up of molecules called

A

molecular element

39
Q

define ‘diatomic’

A

elements made up of molecules containing two atoms.

40
Q

define a single bond

A

when atoms share one pair/2 electrons

41
Q

single bond symbol

A

element-element
eg: (CI-CI)

42
Q

define a double bond

A

when atoms share two pairs/4 electrons

43
Q

double bond symbol

A

element=element
eg: (O=O)

44
Q

define a triple bond

A

when atoms share three pairs/6 electrons

45
Q

triple bond symbol

A

elementΞelement
eg: (NΞN)

46
Q

why do ions have high melting and boiling points

A

because ionic bonds are very strong and it takes a lot of heat energy to break up the lattice. ions also have double the charge so its ionic bonds are stronger.

47
Q

why are ions soluble in water

A

water molecules are able to bond with both the positive and the negative ions, which breaks up the lattice and keeps the ions apart.

48
Q

what is the term for an element that has been dissolved in water

A

aqueous

49
Q

define ‘molten’

A

a substance or element in liquid form

50
Q

why can ions only conduct electricity in molten or aqueous form

A

because the ions become free to move and since they are charged, they can then conduct electricity. (they also gain more charge from the water molecules)

51
Q

why do covalent compounds have low melting and boiling points

A

because the attraction between the molecules is low. so it does not take much energy to break up the lattice and separate them from each other.

52
Q

why are many molecular compounds liquids or gases at room temperature

A

because they have low melting and boiling points.

53
Q

why are many covalent liquids volatile

A

because the attraction between the molecules are low.

54
Q

define ‘volatile’

A

evaporates easily

55
Q

why can’t covalent compounds conduct electricity

A

because covalent compounds have no charged particles.

56
Q

what are the 2 types of molecular structures

A

simple molecular or giant molecular

57
Q

define a simple molecular structure

A

formed from only a few atoms and have strong covalent bonds between the atoms within a molecule.

58
Q

define inTRAmolecular bonds

A

strong covalent bonds between the atoms within a molecule.

59
Q

define inTERmolecular bonds

A

weak bonds between the molecules.

60
Q

why do some covalent compounds have high melting and boiling points and strong inTERmolecular bonds.

A

because they have strong lattice structures and is held in place by 4 strong covalent bonds

61
Q

what are structures like diamonds and silica known as

A

giant covalent structures or macromolecules.

62
Q

why are diamond very hard

A

because each atom is held in place by four strong covalent bonds.

63
Q

why can’t diamonds conduct electricity

A

because there are no ions or free electrons to carry the charge.

64
Q

define ‘allotropes’

A

two forms of the same element.

65
Q

why are diamond and graphite so different

A

because the they have very different structures. (graphite’s structure is a ring of 6 atoms that form flat sheets that lie on top of each other, held together by weak forces)

66
Q

why is graphite so soft and slippery

A

because the sheets
can slide over each other easily.

67
Q

why can graphite conduct electricity but not diamond

A

because each carbon atom has four outer electrons, but forms only three bonds. so the fourth electron is free to move through the graphite, carrying charge.

68
Q

define ‘metallic bonding’

A

when the negatively charged electrons attract all the positive metal ions and bond them together with strong electrostatic forces of attraction as a single unit.

69
Q

how does metallic bonding work

A

electrons in the outer energy level of the atom of a metal move freely throughout the structure they are delocalised forming a mobile ‘sea’ of electrons.

70
Q

why do metals have high melting points

A

because it takes a lot of heat energy to break up the lattice, formed by its strong metallic bonds.

71
Q

define ‘malleable’

A

it means they can be bent and pressed into shape.

72
Q

define ‘ductile’

A

it means they can be drawn out into wires. this is because the layers can slide over each other.

73
Q

why are metals good conductors of heat

A

because the free electrons take in heat energy, which makes them move faster. they quickly transfer the heat through the metal structure.

74
Q

why are metals good conductors of electricity

A

because the free electrons can move through the lattice carrying charge.

Jr 1 - chem (4 decks)

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