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Chemistry > Module 1 > Flashcards

Module 1 Flashcards

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1
Q

pure substance

A

substance that is not contaminated by any other substances

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2
Q

impure substance

A

one substance contaminated with small amounts of one or more other substances.
a mixture

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3
Q

homogenous

A

uniform composition throughout

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4
Q

heterogenous

A

having non uniform composition

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5
Q

element

A

pure substance that cannot be decomposed into simpler substances

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6
Q

compound

A

pure substance that can be decomposed into simpler substances,
for example into elements

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7
Q

an atom

A

smallest particle of an element that is still recognisable as that element

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8
Q

molecule

A

smallest particle of a substance that is capable of separating existence

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9
Q

physical properties of a substance

A

characteristics that we can observe or measure without changing it into a different substance

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10
Q

chemical properties of a substance

A

those associated with the chemical changes or chemical reactions the substance undergoes with it is mixed with other substances, are heated or exposed to light

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11
Q

volatile

A

easily converted into a vapour or that evaporation occurs quite rapidly

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12
Q

density

A

defined as mass per unit volume

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13
Q

filtration

A

method of separating an undissolved solid from a liquid or solution. The solution or liquid that passes through a filter paper is called the filtrate

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14
Q

distillation

A

the process in which a solution or mixture of liquids is boiled, with the vapour formed being condensed back to a liquid in a different part of the apparatus and so separated from the mixture. The liquid collected from a distillation is called a distillate.

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15
Q

fractional distillation

A

process in which a mixture of liquids is separated by being put through many successive distillations (vaporisation and condensations) in one piece of equipment

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16
Q

sedimentation

A

the process in which solids settle to the bottom of a container

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17
Q

decanting

A

the process of carefully pouring off liquid and leaving the solid undisturbed at the bottom of the container

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18
Q

two liquids are immiscible if

A

when they are mixed, they do not for a homogenous liquid

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19
Q

miscible

A

liquids that mix to form a homogenous liquid

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20
Q

metals are elements that

A

solids at room temperature
shiny or lustrous appearance
good conductors of heat and electricity
malleable and ductile
high bp and mp
dense

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21
Q

structure of atom

A

extremely small dense nucleus/core which contains the bulk of the mass of the atom and carries positive electrical charges.
nucleus is surrounded by an electron cloud of rapidly moving and extremely light negatively charged particles

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22
Q

isotopes

A

atoms of the one element that have different numbers of neutrons in their nuclei (although the same number of protons)

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23
Q

chemical properties and physical properties of isotope

A

Isotope of the one element have the same chemical properties and very similar
physical ones

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24
Q

radioactive isotopes

A

spontaneously emit radiation. They are also
called unstable isotopes

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25
Q

what are the 3 radiations emitted from radioisotopes

A

Alpha rays (α) which are helium nuclei
Beta rays (β) which are electrons
Gamma rays (γ) which are a type of electromagnetic radiation like light and
x-rays

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26
Q

nucleur equation

A

shows the disintegration of a radioisotope

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27
Q

what is first, second, third energy level

A

electrons in an atom exist in discrete energy levels through electron configuration
energy shells/energy levels

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28
Q

what are valence electrons in terms of energy level/energy shells

A

highest energy level (outermost energy shell)

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29
Q

orbital

A

volume of space surrounding the nucleus of an atom through which one or two electrons may randomly move

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30
Q

what the orbitals called

A

each main energy level is made up of energy sublevels called spdf sublevels

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31
Q

orbital notation

A

in terms of shells and subshells, 1s

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32
Q

why do electrons get excited

A

An electron in an atom can be given extra energy and so be raised from its ground
state into an excited state
fall back into their ground states, energy is released
in the form of ultraviolet, visible and infrared radiation, photons of light
creates a pattern of lines called emission spectrum

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33
Q

the bohr theory

A

electrons as particles orbiting the nucleus as planets orbit the sun

34
Q

schrodinger’s theory

A

electrons move at extremely high speeds randomly throughout volumes of space around the nucleus called orbitals

35
Q

periodicity

A

regular recurrence of events or properties

36
Q

atomic radius trends

A

decreases along the period - attraction between electrons in shells and protons in nucleus pulls shells closer to nucleus

increases down a group- increase in shells

37
Q

first ionisation energy

A

the energy required to remove an
electron from an atom

38
Q

equation for ionisation energy

A

M(g) → M+(g) +e-

39
Q

trends of first ionisation energy on periodic table

A

increases across period: as attraction between valence electrons and nucleus increases, radius gets smaller and harder to remove valence electrons
decreases down group: more shells means less attraction of valence electrons to nucleus, making ti easier to remove outmost electrons

40
Q

electronegativity of an element

A

a measure of the ability of an atom of that
element to attract bonding electrons towards itself in compounds.
the higher the electronegativity the stronger the attraction for bonding electrons

41
Q

trends of electronegativity on periodic table

A

increases across period: change from metal to non metal…
decreases down group: increase in metallic character…

42
Q

state if the following are compressible/incompressible and how they fit ina container
solids
liquids
gases

A

solids: incompressible and holds its shape
liquids: incompressible and fills the shape of the container
gases: compressible and fills the shape of the container

43
Q

examples of physical properties

A

appearance, colour, magnetism, mp, bp, density, malleability, ductility, solubility in water

44
Q

examples of chemical properties

A

rate of reactivity to water, acids, and substances, oxygen, rate burnt by oxygen, if its acidic or basic

45
Q

separation techniques based on bp

A

evaporation, distillation, fractional distillation

46
Q

separation techniques based on density

A

decanting, seperating funnel, centrifuging

47
Q

separation techniques based on particle size

A

sieving, filtration

48
Q

reason for each radioactive type of decay

A

alpha: nuclei have too few neutrons to be stable
beta; nuclei has too many neutrons to be stable
gamma: unstable atom releasing energy

49
Q

why is carbon 12 important

A

its used as the standard from which atomic masses of all nuclides are measured

50
Q

what are shells also called

A

energy levels

51
Q

what group numbers are each subshell

A

s: Group 1-2
p: group 13-18
d: group 3-12
f: lanthanides and actinides

52
Q

What does bonding depend on?

A

The difference in electronegativity
If big: electron will be transferred and make an ionic compound
If small: electrons will be shared and make a covalent compound

53
Q

Do metals comonnly lose or gain electrons

A

They lose since most charges are +1 to +3

54
Q

the metallic bonding model

A

describes metals as a metallic structure which consists of a regular arrangement of stable, positively charged metal ions, called cations, surrounded by a ‘sea’ of freely moving delocalised valence electrons. The metal atoms achieve stability by releasing their valence electrons to become the surrounding ‘sea’.

55
Q

metallic bonds

A

electrostatic attraction between the cations and the freely moving electrons

56
Q

characteristics of ionic compounds

A

brittle, hard (resistant to scratching, high mp, cant conduct electricity in solid state but can in liquid or aqueous state

57
Q

ionic bonding model

A

ionic networks that consists of a regular arrangement of metal cations and negativitely charged non-metal ions called anions
electronegativity difference is high

58
Q

ionic bonds

A

electrostatic attractions between the oppositely charged ions

59
Q

electrovalency

A

charge of an ion

60
Q

what type of ion is metals

A

cations

61
Q

what type of ion is non-metals

A

anion

62
Q

why do covalent bonds share electrons

A

since non metals have similar electronegativity and therefore result to share electrons

63
Q

why do ionic bonds transfer electrons

A

since metals and non metals have a big difference in electronegativity and therefore attract each others electrons.

64
Q

discrete molecules

A

formed containing fixed numbers of atoms. diatomic molecules

65
Q

intramolecular forces

A

forces that hold atoms together within a molecule

66
Q

intermolecular forces

A

forces that exist between molecules

67
Q

molecular shapes

A

linear, bent, trigonal planar, tetrahedral, pyramidal

68
Q

properties of covalent molecular substances

A

low mp and bp: weak intermolecular forces (substnce must be cooled to form fixed lattice)
non-conduction fo electrcity in solid or molten states: no free moving particles
softness

69
Q

covalent network

A

a three dimensional network of atoms fixed in place, held together by strong covalent bonds extending through lattice
covalent network structure: forms when covalent bonds extend throughout an entire substance (diamond)
covalent layer network: forms when covalent bonds extend throughout layer in a substance, weak dispersion forces between layers (graphite)

70
Q

explanation for properties of metallic substances

A

good conductors of heat and electricity: delocalised electrons transfer charge and thermal energy
high mp and bp: strong metallic bonding extending throughout the lattice
dense: ions tightly packed in the lattice
malleable and ductile: distortions does not distrupt the metallic bonding
lustrous: delocalised electrons cause reflection of light

71
Q

explanation of properties of ionic substances

A

non conductors of electricity when solid: ions firmly bound in the lattice, so no moving charged particles
conductors when molten or aqueous: ions free to move
high mp and bp: strong ionic bonding extending throughout the lattice
hard: ions strongly bound in the lattice
brittle: distortion causes repulsion between ions of like charge

72
Q

explanation of properties of covalent molecular substances

A

non conductors of electricity unless reacted with water to produce ions: molecules are uncharged and electrons are localised in covalent bonds or on the atoms
low mp and bp: weak forces between molecules
soft solids, liquids or gases: weak forces between molecules

73
Q

explanation of properties of covalent network substances

A

non conducters when solid or molten: electrons localised in covalent bonds or on the atoms
very high mp: atoms strongly bound in the lattice
hard: strong covalent bonding extending throughout the lattice
brittle: distortion breaks covalent bonds

74
Q

form a flow chart of different bonds

A

see in onenote

75
Q

covalent molecular compounds

A

neutral molecules held together by weak intermolecular forces
strong covalent bonds within molecule but forces between molecules are weak

76
Q

why is graphite an excluded example of a covalent network bond?

A

is has layers of covalent bonds that have weak intermolecular bonds but strong intramolecular bonds
they can conduct electricity since there are extra electrons forming clouds between the layers,

77
Q

what are the two types of pairs in VSEPR

A

bonding pairs: between two atoms
lone pairs: not involved in bonding

78
Q

what is the VSEPR theory

A

valence shell electron pair repulsion

79
Q

why do lone pairs take up more space

A

lone pair electrons repel each other more than bonding pairs

80
Q

what is diamond

A

a carbon covalent network
each carbon atom is covalently bonded to four other carbon atoms in a tetrahedral arrangement
hard, high mp, not conductor of electricity,

81
Q

what is silicon dioxide

A

a covalent network
each Si atom joined to 4 oxygen atoms
main substance in rocks, when pure: quartz

82
Q

trends of state of matter at room temperature

A

melting points increase across periods 1-3 from groups 1-14 then drastically drop for groups 15-18

Chemistry (5 decks)

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