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Chemistry > Atomic structure & states of matter, Group 1 & 7 + redox, Writing formula and balancing equations , Reactivity Series > Flashcards

Atomic structure & states of matter, Group 1 & 7 + redox, Writing formula and balancing equations , Reactivity Series Flashcards

- Atomic structure & states of matter - Group 1 & 7 + redox - Writing formula and balancing equations - Reactivity Series

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1
Q

what 3 things affect the strength of attractive forces in a material?

A
  • the material
  • the temperature
  • the pressure
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2
Q

describe the movement of particles in solids

A
  • particles vibrate about a fixed point
  • the hotter a solid becomes, the more they vibrate.
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3
Q

in a solid the particles don’t ____ from their positions, so all solids keep a definite ____ and ______.

A
  • move
  • shape
  • volume
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4
Q

describe the structure / forces of attraction in solids

A
  • strong forces of attraction between particles
  • holds them close together
  • in fixed positions
  • forms a regular lattice arrangement
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5
Q

describe the structure of liquids

A
  • weak attractive forces between particles
  • random arrangement
  • free to move past each other, but tend to stick closely together
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6
Q

liquids have a definite ____ but don’t keep a definite ____. They will ____ to fill the bottom of their container.

A
  • volume
  • shape
  • flow
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7
Q

describe the movement of particles in liquids

A
  • particles are constantly moving with random motion
  • the hotter a liqud becomes, the faster they vibrate
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8
Q

describe the forces of attraction in gases

(and their movement)

A
  • very weak forces of attraction between particles
  • so they are far apart
  • particles are free to move
  • and travel in straight lines.
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9
Q

gases don’t keep a definite ____ or volume and will always ____ any container.

A
  • shape
  • volume
  • fill
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10
Q

describe the movement of gas particles

A

gas particles move:
- constantly
- with random motion
- and travel in straight lines

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11
Q

what happens to solids, liquids and gases when heated?

A

solids: vibrate more (causing solids to expand slightly when heated)
liquids: particles move faster (causing liquids to expand slightly when heated)
gases: particles move faster. (When heated, gases either EXPAND or their PRESSURE INCREASES.)

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12
Q

why does ammonia gas diffuse quicker than hydrogen chloride gas?

A

the particles of ammonia are SMALLER nad LIGHTER than the particles of hydrogen chloride, so they diffuse through the air more quickly.

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13
Q

why does/can diffusion happen in liquids and gases (but not solids)?

A

due to the RANDOM MOVEMENT of particles (particles in solids are in fixed positions, so they ca’t move, therefore diffusion can’t take place)

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14
Q

relative mass of a proton

A

1

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15
Q

relative mass of a neutron

A

1

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16
Q

relative mass of an electron

A

0.0005

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17
Q

relative charge of a proton

A

+1

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18
Q

relative charge of a neutron

A

0

(neutral)

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19
Q

relative charge of an electron

A

-1

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20
Q

what does the nucleus of an atom contain

A

protons and neutrons (if there are any neutrons)

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21
Q

what is the overall charge of the nucleus? why?

A

+ive, because of the protons

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22
Q

electrons move around the ____ in energy levels called ____ ?

A
  1. nucleus
  2. shells
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23
Q

why do neutral atoms have no charge overall?

A

because there is an equal number of protons and electrons, so their charges cancel each other out

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24
Q

protons and electrons have an ____ but ____ charge

A
  • equal
  • opposite
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25
Q

what defines an atom/element?

A

the number of protons

(the atomic number –> number at the bottom)

26
Q

what is an ion?

A

an ION is an ATOM with a CHARGE.
the atom becomes charged by gaining or losing electrons.

27
Q

what does the atomic number tell you?

A

number of protons

(also number of electrons since number of protons = number of electrons)

28
Q

what does the mass number tell you?

A

the total of protons and neutrons in the atom

29
Q

what is the overall charge of any ionic compound?

A

0

(so all -ive charges must balance all +ive charges)

30
Q

how can you work out the formula for an ionic compound?

A

swap and drop method

31
Q

state symbol for solid

A

(s)

32
Q

state symbol for liquid

A

(l)

33
Q

state symbol for gas

A

(g)

34
Q

state symbol for aqueous

(dissolved in water)

A

(aq)

35
Q

what is the trend in reactivity going DOWN Group 1?

A

as you go DOWN the group, reactivity INCREASES

36
Q

(describe and) explain the trend in reactivity going down group 1

A
  • going down the group, reactivity increases
  • electrostatic attraction becomes weaker because there are more electron shells
  • outer shell is less strongly attracted to the nucleus
  • therefore it is EASIER to LOSE an electron (and obtain a full outer shell)
37
Q

what name is given to the group 1 metals? why?

A

the alkali metals because they react with water to form an alkaline solution

38
Q

word equation for sodium (or any other group 1 metal) with water

A

sodium + water –> sodium hydroxide + hydrogen

39
Q

symbol equation for sodium (or any other group 1 metal) with water

A

2Na (s) + 2H2O (l) –> 2NaOH (aq) + H2

(2’s in bold should be subscript)

40
Q
  1. word equation for rection of lithium and oxygen
  2. sybol equation for reaction of lithium and oxygen
A
  1. lithium + oxygen –> lithium oxide
  2. 2Li + O2 –> Li2O
41
Q

complete the equation:
sodium + water –> ?

Group 1

A

sodium hydroxide + hydrogen

42
Q

Group 7: as the ____ number of the halogens increases”, the elements have a _ colour and a ____ boiling point.

“i.e. going DOWN the group

A
  • atomic
  • darker
  • higher
43
Q

chlorine is a fairly reactive, poisonous, ____ gas.

A

green

44
Q

bromine is a poisonous, ___-___ liquid, which gives off a ____ vapour at room temperature.

A
  • red-brown
  • orange
45
Q

iodine is a _ _ crystalline solid which gives off a _ vapour when heated.

A
  • dark grey
  • purple
46
Q

what physical state is chlorine at room temperature?

group 7

A

gas

47
Q

what physical state is bromine at room temperature?

group 7

A

liquid

48
Q

what physical state is iodine at room temperature?

group 7

A

solid

49
Q

which is more reactive, astatine or iodine? explain your answer (3 marks)

group 7

A

iodine…
- reactivity decreases going down group 7 and astatine is lower down
- electrostatic attraction becomes weaker because there are more electron shells
- outer shell is less strongly attracted to the nucleus
- harder for astatine than iodine to gain an electron in the outermost shell.

50
Q

what is the trend in reactivity going DOWN group 7?

A

going DOWN the group, reactivity DECREASES

51
Q

what is a displacement reaction?

A

when a more reactive element displaces a less reactive element from its compound

52
Q

when something is oxidised does it gain or lose electrons?

A

electrons are LOST

(OIL RIG)

53
Q

when something is reduced does it gain or lose electrons?

A

electrons are GAINED

(OIL RIG)

54
Q

complete the equation:
chlorine + potassium iodide –> ?

displacement reactions

A

iodine + potassium chloride

55
Q

what is oxidation?

2 answers

A
  1. when oxygen is gained
  2. the loss of electrons
56
Q

what is reduction?

2 answers

A
  1. when oxygen is lost
  2. the gain of electrons
57
Q

what happens to an oxidising agent?

A

it ACCEPTS electrons and GETS REDUCED

58
Q

what happens to a reducing agent?

A

it DONTATES electrons and GETS OXIDISED

59
Q

acid + metal –> ?

reactions of metals

A

salt + hydrogen

60
Q

you can use the reactions of different metals with dilute acids to work out how reactive they are. the more __ the metal, the __ the reaction will go.

A
  • reactive
  • faster
61
Q

describe an experiment to investigate the difference in reactivity of a variety of metals.

A
  • first, set up 3 boiling tubes and fill them with equal volumes of dilute HCl (or dilute H2SO4).
  • then place pieces of magnesium, zinc and iron in separate test tubes. ensure the size and shape of the metal pieces are the same.
  • the speed of the reaction is indicated by the rate at which hydrogen bubbles are given off.

Chemistry (10 decks)

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