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Chemistry > Unit 2 > Flashcards

Unit 2 Flashcards

1
Q

Define element

A

An element contains 1 type of atom

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2
Q

Define mixture

A

2 or more different types of atoms not chemically bound

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3
Q

Define compound

A

2 or more different types of atoms chemically bound

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4
Q

Define isotopes

A

different atoms of the same element that have the same number of protons and electrons but a different numbers of neutrons

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5
Q

Formula for isotopes mass

A

[(atomic mass x percentage its found) + (atomic mass x percentage its found)] / 100

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6
Q

Define metallic bonds

A

electrostatic attraction between negative delocalized electrons and positive metal nuclei

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7
Q

Define ionic bonds

A

electrostatic attraction between positive metal ions and negative non metal ions

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8
Q

Define covalent bonds

A

electrons shared between non-metal atoms

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9
Q

Define ion

A

Charged particle

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10
Q

Are melting and boiling points for ionic and metallic compounds high or low? Why?

A

High because there are many bonds between the positively charged ions and negatively charged ions and the electrostatic forces are strong

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11
Q

Are melting and boiling points for covalent molecules high or low? Why?

A

Low because the intermolecular forces are weak

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12
Q

Are intermolecular forces strong or weak? What is the effect of this?

A

Weak. it affects substances by making it easy to change states and making it have a low melting and boiling point

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13
Q

what are the structures called when the bonds are in 3 directions?

A

giant metallic lattices and giant ionic lattices

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14
Q

define simple molecules

A

singular molecules (except sand and carbon bonded molecules)

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15
Q

What is the state of fluorine at room temperature? what colour is it?

A

gas. yellow

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16
Q

What is the state of chlorine at room temperature? what colour is it?

A

gas. yellow-green

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17
Q

What is the state of bromine at room temperature? what colour is it?

A

liquid. brown

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18
Q

What is the state of iodine at room temperature? what colour is it?

A

solid. brown-black

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19
Q

state 4 facts about diamond

A

-Made of carbon
-doesn’t conduct electricity because it doesn’t have delocalized electrons
-Not soluble
-4 covalent carbon bonds

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20
Q

state 4 facts about graphite

A

-made of carbon
-does conduct electricity because it has delocalized electrons so charge can flow
-Not soluble
-3 covalent carbon bonds
-it is soft and slippery

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21
Q

state 3 facts about silicon dioxide

A

-SiO2
-doesn’t conduct electricity because it doesn’t have delocalized electrons
-Not soluble

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22
Q

Can ionic compounds conduct electricity? why?

A

Only when molten or aqueous because ions are only free to move when molten or an aqueous solution

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23
Q

Can covalent molecules conduct electricity? why?

A

No because there are no free to move ions (except graphite)

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24
Q

Can metallic molecules conduct electricity? Are the malleable and ductile? why?

A

Yes because the layers can slide over one another and can move

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25
Q

Can ionic compounds dissolve in water?

A

Most do, Yes

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26
Q

Can covalent molecules dissolve in water?

A

mostly no, No

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27
Q

Can metals dissolve in water? why?

A

No because the bonds are strong

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28
Q

what is the relationship between group 1 metal and water?

A

group 1 metals are reactive with water but are not soluble in water

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29
Q

define independent variable and give 1 example

A

usually on x axis, the thing that changes (concentration of salt in osmosis)

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30
Q

define dependent variable and give 1 example

A

usually on y axis, the thing that we measure (the length of potato in osmosis)

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31
Q

what should the sentence structure be for describing trends on a graph?

A

As x-axis goes up, what happens to y-axis?

32
Q

as the atomic radius gets bigger, does it get easier or harder to remove electrons? why?

A

Easier. because the electrons are further away from the nucleus so there is less attraction and there are more shells which is more shielding so theres lower attraction

33
Q

as the atomic radius gets bigger is it more reactive or less reactive?

A

more reactive

34
Q

as the atomic radius gets bigger, does it get harder or easier to attract electrons? why?

A

harder because the electrostatic attraction is weaker (its further apart and more shielding)

35
Q

define atom

A

smallest unit of matter that can’t be broken down more

36
Q

why do isotopes have the same chemical properties?

A

because they have the same electronic configuration

37
Q

define ductile and is it a physical or chemical property?

A

can be pulled into a wire, physical property

38
Q

define malleable and is it a physical or chemical property?

A

can be hammered into a shape, physical property

39
Q

define high conductivity

A

can conduct thermal energy and electricity

40
Q

why can substances transfer energy? (electrons)

A

because electrons are free to move

41
Q

what are word equations? (use example to explain)

A

2.8.1 + 2.8.7 = 2.8+ + 2.8.8-

42
Q

what are symbol equations? (use example to explain)

A

Na + Cl2 = NaCl

43
Q

what does the atomic number tell us?

A

how many protons there are

44
Q

what does the atomic mass tell us?

A

mass of / number of protons + neutrons

45
Q

formula for number of neutrons

A

atomic mass - atomic number

46
Q

difference between element and ion

A

an element is a not charged particle and an ion is a charged particle

47
Q

define occupied electron shells

A

shells with electrons in the shells

48
Q

what is the pattern in a metallic bond?

A

electrons are free to move and delocalized and protons have a regular pattern

49
Q

what is the physical properties of mass and density of isotopes?

A

have different mass and density because number of neutrons is different

50
Q

does an element and atom have a charge?

A

no

51
Q

does an ion have a charge?

A

yes

52
Q

formula for atomic mass

A

number of protons + number of neutrons

53
Q

define radioactive

A

nucleus is unstable

54
Q

as the atomic radius gets smaller, what happens to the energy level?

A

decreases (get lower)

55
Q

what are 3 ways to say ‘how electrons are arranged in shells’

A

-electron arrangement
-electron distribution
-electronic configuration

56
Q

define impurities

A

unwanted substance mixed with wanted usbstsance

57
Q

define pure substance

A

only particles of own substance/no particles of other substances mixed in

58
Q

define brittle

A

breaks easily when struck

59
Q

define sonorous

A

makes a ringing noise when struck

60
Q

are metals brittle? are metals sonorous? are metals good conductors? are metals ductile? are metals malleable?

A

no, no, yes, yes, yes, yes

61
Q

define diatomic

A

elements made up of molecules containing 2 atoms

62
Q

do molecular substances have low or high melting and boiling points? why?

A

low because forces between molecules (intermolecular forces) in the lattice are weak

63
Q

what are halogens?

A

most reactive non metals (group 7)

64
Q

what are noble gases?

A

most unreactive non metals (group 8)

65
Q

what groups have the most reactive metals?

A

1 and 2

66
Q

what are magnetic metals?

A

Fe, Co, Ni

67
Q

define valency electrons

A

The electrons in an atom’s outer shell

68
Q

What happens to a radioactive nucleus

A

Atom breaks down naturally (decays) giving our radiation in the form of rays and particles and a large amount of energy

69
Q

What are 3 uses of radioisotopes?

A

-To check for leaks
-to treat cancer
-to kill germs and bacteria

70
Q

What type of electron decides how an element reacts?

A

Valency electrons

71
Q

Why do atoms form bonds?

A

To have a stable outer shell

72
Q

Define ionic compound

A

Substance made of ions

73
Q

Define compound ions

A

Ions formed from a groop of bonded atoms

74
Q

Define molecules

A

A group of atoms held together by covalent bonds

75
Q

Define covalent compounds

A

Atoms of different elements sharing electrons

76
Q

What shape are molecules?

A

Tetrahedral

77
Q

3 properties of ionic compounds

A

-good conductor if aqueous or molten (bad if solid)
-soluble in water (generally)
-high melting and boiling point

Chemistry (6 decks)

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