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Chemistry Whole NAT5 Course > UNIT 1 A > Flashcards

UNIT 1 A Flashcards

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1
Q

Rates of reaction equation

A

delta Q/delta T

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2
Q

Name 4 things that can impact the rate of a reaction

A

temperature increase= faster reaction
particle size decrease= faster reaction
concentration increase= faster reaction
addition of catalyst= faster reaction

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3
Q

Name 3 signs of a chemical reaction

A

change in colour, gas given off, solid being formed

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4
Q

definition of a catalyst

A

catalysts speed up reactions and remain unchanged

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5
Q

how can the process of a chemical reaction be followed

A

by measuring the change in concentration, mass or volume

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6
Q

in chemistry do yo use a line of best fit or join the dots on a line graph?

A

line of best fit

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7
Q

what are the units of average rate dependant on?

A

the quantity being measured from the y axis and the units of time used in the graph

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8
Q

What does nuclide notation tell us?

A

the symbol, atomic number and mass of an atom

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9
Q

in nuclide notation placement, where do we find the mass of an atom

A

ABOVE the symbol

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10
Q

what is the position in atoms of protons, neutrons and electrons

A 
protons/neutrons= inside nucleus
electrons= orbiting the nucleus
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11
Q

charge of protons, neutrons and electrons

A 
p= +1
n= no charge
e= -1
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12
Q

mass of protons, neutrons and electrons

A 
p= 1
n= 1
e= 0
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13
Q

definition of an isotope

A

atoms with same atomic number but a different mass number

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14
Q

what is the RAM

A

relative atomic mass- the average mass of the isotopes of an element

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15
Q

why is the mass number different between isotopes

A

because they have a different number of neutrons

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16
Q

in electron arrangement what do metals lose and non metals gain to obtain a full outer shell

A

electrons

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17
Q

why do atoms want a full outer shell of electrons

A

to become stable like a noble gas

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18
Q

what number of electrons is a full outer shell

A

8

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19
Q

3 main types of bonding and what elements they represent

A

covalent- non metals only
ionic- metals and non metals
metallic- metals only

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20
Q

definition of covalent bonding

A

the attraction between two non metal atoms, where a pair of electrons is shared in the bond

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21
Q

how are the electrons held in a covalent bond

A

by both nuclei, forming an extremely strong bond

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22
Q

WHAT IS A COVALENT MOLECULE

A

a group of non metal ions held together by covalent bonds

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23
Q

when do you draw a circle electron cloud diagram

A

if the element is helium or hydrogen

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24
Q

in electron cloud diagrams does the drawing of the bond include both electrons?

A

YES

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25
Q

DIATOMIC ELEMENTS ?

HINClBrOF

A

HYDROGEN, IODINE, NITROGEN, CHLORINE, BROMINE, OXYGEN, FLOURINE

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26
Q

NAME THE 4 DIFFERENT SHAPES OF MOLECULES

A

linear, angular, trigonal pyramidal, tetrahedral

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27
Q

formula for calculating time in half life

A

half live multiplied by no. of half lifes

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28
Q

formula for no. half lifes

A

time divided by 1 half life

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29
Q

formula for half life of a sample

A

time divided by no. half lifes

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30
Q

moles formula

A

n=cv

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31
Q

three step calcs steps…

A
  1. no. moles 2. mole ratio 3. mass
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32
Q

definition of standard solution

A

a solution of accurately known concentration

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33
Q

what stops beta emission

A

ALUMINIUM

34
Q

What stops alpha emmision

A

paper

35
Q

what stops gamma emission

A

concrete

36
Q

mass of alpha radiation (shown by nuclide notation)

A

4

37
Q

mass of beta radiation

A

0

38
Q

mass of gamma radiation

A

0

39
Q

charge of alpha radiation

A

2+

40
Q

charge of beta radiation

A

-1

41
Q

charge of gamma radiation

A

0

42
Q

how can unstable nuclei become stable?

A

by giving out alpha, beta or gamma radiation

43
Q

half life definition

A

the time taken for the activity or mass of a radioactive sample to half

44
Q

I terms of cloud diagrams, what type of bond does oxygen form?
(rarer than most bonds)

A

a double bond

45
Q

how many elements in a bond does a tetrahedral shape represent

A

5

46
Q

how many elements does a trigonal pyramidal shape represent?

A

4

47
Q

what is a covalent network?

A

an extremely large structure of non metal atoms that extend in 3 dimensions

48
Q

example of a covalent network structure?

A

the element carbon (graphite & diamond)

49
Q

when are ions made

A

when atoms lose or gain electrons and become pos or neg

50
Q

what is ionic bonding

A

the attraction between positive and negative ions

51
Q

when metals lose electrons, do they form positive or negative ions
(for example: Mg ^2)

A

POSITIVE

52
Q

when non metals gain electrons do they form positive or negative ions?

A

negative

even though they have GAINED electrons they are still negative- still a minus sign!

53
Q

what structures do ionic compounds exist as?

A

giant lattice structures

54
Q

what do substances need to be able to conduct

A

charged particles which are free to move and carry the electricity

55
Q

do covalent substances conduct and why?

A

no, because they have no free, charged particles which can carry electricity

56
Q

why can graphite conduct unlike all other covalent substances

A

because it has delocalised electrons whichcan move between carbon atoms

57
Q

do covalent substances dissolve

A

not in water but in other liquids such as petrol, yes

58
Q

what page in data book can you find which ionic substances are soluble

A

5

59
Q

why do ionic substances dissolve ?

A

because water can squeeze between the ions

60
Q

why do ionic, metallic and covalent networks have a high boiling point b

A

because they are held by very strong bonds

61
Q

what is the combustion equatin

A

hydrocarbon + O2 = energy, CO2, H2O

62
Q

state whether metallic, ionic and covalent substances are soluble in water?

A 
m= no
i= yes
c= no
63
Q

state the MP/BP of molecule and networks

A 
m= low
n= high
64
Q

what is the meaning of the TETRA prefix

A

4

65
Q

what is the meaning of the PENTA prefix

A

5

66
Q

what does the ionic formula of a compound tell us that other formulas dont?

A

the valency of the atoms (=the charge)

67
Q

where do acids come from?

A

non metal oxides dissolving in water

68
Q

what is produced when ANY fossil fuels burns (reacts with oxygen)

A

SO2 and CO2

69
Q

what do SO2, CO2 AND NO3 all contribute to?

A

acid rain

70
Q

descibe the concentration of H+ and OH- ions ins an acidic solutions

A

H+>OH-

71
Q

if a metal oxide is soluble what will it dissolve in water to produce?

A

an alkali

72
Q

if a metal oxide is insoluble what will happen

A

the pH will not change

73
Q

name the three salts we use when naming salts and what they =

A 
hydrochloric= chloride
sulfuric= sulphate
nitric= nitrate
74
Q

what three bases can acids react with in neutralisation reactions

A

metal hydroxides, metal oxides, metal carbonates

75
Q

what do acids with metal carbonates make

A

salt+ water+ CO2

76
Q

when naming salts, what does the first part of the name come from?

A

the metal of the base

77
Q

name the three basic steps for neutralisation

A

1) REACTION- add carbonate until gas is no longer being produced
2) FILTRATION- filter paper to remove excess copper carbonate
#3) EVAPORATION- to remove any water leaving you with the salt

78
Q

what type of salts are produced by neutralisation reactions? and what reaction would produce the opposite

A

insoluble salts and precipitation reactions

79
Q

when will a precipitate form

A

if there is a combination of metal and non metal ions in a reaction which is insoluble

80
Q

what is the concentration of an AQUEOUS solution

A

the mass of the solute dissolved in 1L of water

Chemistry Whole NAT5 Course (2 decks)

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