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N5 Chemistry > Unit 1 > Flashcards

Unit 1 Flashcards

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1
Q

list 4 factors that can speed up the rate of a reaction

A
  1. increasing concentration
  2. increasing surface area - decrease particle size
  3. increase temperature
  4. use a catalyst
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2
Q

formula for rate of reaction

A

Average rate = change in quantity/change in time

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3
Q

why does that average rate of a reaction decrease over time?

A

the reactants are being used up so the concentration of reactants are decreasing

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4
Q

what is a catalyst?

A

a substance that speeds up a chemical reaction but is not used up by the reaction

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5
Q

how are elements arranged in the periodic table?

A

in order of increasing atomic number

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6
Q

how are elements in the same group similar?

A
  • they have the same number of outer electrons
  • they have similar chemical properties
  • they have the same valency
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7
Q

describe an atom

A

a nucleus containing protons and neutrons with electrons in orbit

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8
Q

what is the mass number of an atom?

A

the number of protons + neutrons

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9
Q

what is the atomic number of an atom?

A

the number of protons

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10
Q

how do you work out the number of neutrons in an atom?

A

mass number - the atomic number

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11
Q

what is the mass of an electron?

A

an amount so small its not worth working out

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12
Q

what is the charge of an electron?

A

-1

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13
Q

what is the mass of a proton?

A

1 atomic mass unit

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14
Q

what is the charge of a proton?

A

+1

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15
Q

what is the mass of a neutron?

A

1 atomic mass unit

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16
Q

what is the charge of a neutron?

A

0

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17
Q

what are isotopes?

A

atoms with the same atomic number but different mass number ( they have different numbers of neutrons)

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18
Q

what is the relative atomic mass of an element?

A

the average mass of an element

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19
Q

what is a covalent bond?

A

a shared pair of electrons holding non-metal atoms together

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20
Q

how are atoms in a covalent bond held together?

A

by the attraction between the positive nuclei and the shared pair of electrons

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21
Q

list the 7 diatomic elements

A
  • nitrogen
  • oxygen
  • fluorine
  • hydrogen
  • iodine
  • bromine
  • chlorine
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22
Q

what does diatomic mean?

A

two atoms covalently bonded

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23
Q

what shape would a molecule with the formula XY have?

A

linear

24
Q

what shape would a molecule with the formula XY^2 have?

A

angular

25
Q

what shape would a molecule with the formula XY^3 have?

A

trigonal pyramidal

26
Q

what shape would a molecule with the formula XY ^4 have?

A

tetrahedral

27
Q

what is an ion?

A

an atom that has gained or lost electrons in charge ( they do this to be stable like the noble gasses)

28
Q

ionic compounds are usually made from a metal and non-metal. which ion will be positively charged?

A

metal ion = positive

non-metal ion = negative

29
Q

what is an ionic bond?

A

an electrostatic attraction between positive and negative ions

30
Q

what structure do ionic compounds have?

A

crystal lattice

- each positive ion surrounded by a negative ion and each negative ion surrounded by positive ions

31
Q

in general, do ionic substances have high or low melting and boiling points?

A

high

because strong bonds must be broken which requires a lot of energy

32
Q

why do ionic substances only conduct electricity when heated until a liquid or in a solution?

A

because when they are liquid or are in a solution ions are free to move so the substance can conduct electricity

33
Q

what happens at the electrodes when an ionic compound is electrolysed?

A

at the electrode the ion gains or loses electrons

the ion is drawn to the oppositely charges electrode

34
Q

do ionic compounds usually dissolve in water?

A

yes

35
Q

what type of bonding is present in substances that can conduct electricity without decomposing?

A

metallic

36
Q

why can metals conduct electricity?

A

the electrons are delocalised so they are free to move

37
Q

do covalently bonded substances usually conduct energy?

A

no

because there are no free charged particles free to move

38
Q

what is the usual ending for a compound containing only 2 elements?

A

…ide

iron chloride

39
Q

what does the compound ending in …ate or …ite mean?

A

oxygen is present

40
Q

what is pH?

A

a measure of hydrogen ion concentration in a solution

41
Q

what pH would a solution of equal concentrations of hydrogen and hydroxide ions have?

A

pH 7

42
Q

what pH would a solution with a higher concentration of hydrogen ions than hydroxide ions have?

A

pH 1-6 (acid)

43
Q

what pH would a solution with a higher concentration of hydroxide ions than hydrogen ions have?

A

pH 8-14 (alkaline)

44
Q

why is water neutral? (pH 7)

A

when the molecules separate it makes equal concentrations of hydrogen and hydroxide ions

45
Q

what pH will a solution of a soluble non-metal oxide be?

A

less than 7

46
Q

what pH will a solution of soluble metal oxides be?

A

more than 7

47
Q

what are bases?

A

a substance that can react with acids and neutralise them

48
Q

what is an alkali?

A

a base that dissolves in water

49
Q

what is a neutralisation reaction?

A

the reaction of an acid with a base that results in the pH moving towards 7.

50
Q

complete the equation

metal oxide + water =

A

metal hydroxide

51
Q

complete the equation

metal oxide + acid =

A

salt + water

52
Q

complete the equation

metal hydroxide + acid =

A

salt + water

53
Q

complete the equation

metal carbonate + acid =

A

salt + water + carbon dioxide

54
Q

which salts are made from

  • hydrochloric acid
  • nitric acid
  • sulphuric acid
  • ethanoic acid
A
  • chloride
  • nitrate
  • sulphate
  • ethanoate
55
Q

what effect on pH does adding water to an acid have?

A

increases it

56
Q

what do you get when an acid reacts with a metal?

A

salt + hydrogen

57
Q

what effect on pH does anything water to an alkili have?

A

decreases it

N5 Chemistry (3 decks)

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