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Chemistry > Atomic structure and the periodic table > Flashcards

Atomic structure and the periodic table Flashcards

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1
Q

what are atoms?

A

make up all substances and are the smallest part of an element that can exist

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2
Q

what are compounds?

A

a substance made of two or more elements chemically bonded together

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3
Q

what is an element?

A

a substance made up of one type of atom only

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4
Q

what is a mixture?

A

two different substances that are not chemically bonded together

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5
Q

how can mixtures be separated?

A

filtration, crystallisation, distillation, chromatography

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6
Q

what does soluble mean?

A

a substance that can dissolve in a liquid

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7
Q

what is a solute?

A

a solid which can dissolve

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8
Q

what does insoluble mean?

A

a substance that cannot dissolve in a liquid

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9
Q

what is a solution?

A

what is made up when a solid has dissolved in a liquid

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10
Q

radius of a nucleus

A

1 x 10 -14 m

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11
Q

relative mass of a proton

A

1

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12
Q

relative mass of a neutron

A

1

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13
Q

relative mass of an electron

A

very small

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14
Q

relative charge of a proton

A

+1

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15
Q

relative charge of a neutron

A

0

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16
Q

relative charge of an electron

A

-1

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17
Q

why do atoms have no charge?

A

same number of protons and electrons
same size charge - cancels out

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18
Q

radius of an atom

A

1 x 10 -10 m

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19
Q

what does the top number on periodic table mean?

A

mass number

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20
Q

what does the bottom number on an element mean?

A

atomic number

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21
Q

how do you calculate the number of neutrons?

A

mass number - atomic number

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22
Q

how do you calculate the number of protons

A

atomic number

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23
Q

how do you calculate the number of electrons

A

atomic number

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24
Q

what makes atoms an element?

A

same number of protons in all

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25
Q

what year did john dalton create his model of the atom?

A

1800s

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26
Q

what was john daltons atom like?

A

tiny spheres
atoms of particular element are all identical
they could combine to make compounds

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27
Q

what was jj thompsons model of the atom

A

plum pudding model
discovered the electron
ball of positive charge with electrons embedded

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28
Q

when was jj thomson’s plum pudding model discovered

A

1897

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29
Q

when was john daltons model of the atom discovered

A

1800s

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30
Q

what was geiger and marsdens experiment about the atom

A

fired alpha particles at a thin sheet of gold
expected alpha particles to pass straight through, but they didn’t

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31
Q

what was the result of the alpha particle experiment

A

most alpha particles passed straight through = lots of empty space

some particles were deflected = nucleus with positive charge

some particles bounced back = small, lots of mass, in the centre

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32
Q

which year was the alpha particle experiment

A

1910

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33
Q

what did ernest rutherford discover about the atom

A

new model
solid positive nucleus
negative electrons in orbit around it

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34
Q

which year did ernest rutherford discover his new atom

A

1911

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35
Q

which year did niels bohr discover his atom

A

1914

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36
Q

what did niels bohr discover about the atom

A

electrons must be orbiting the nucleus at a set distance called shells

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37
Q

what did james chadwick discover about the atom

A

third particle called a neutron
found in the nucleus

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38
Q

which year did james chadwick discover the neutron

A

1932

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39
Q

what is the atomic number

A

number of protons

40
Q

what are isotopes

A

atoms of the same element with the same number of protons and electrons but a different number of neutrons

41
Q

what are the properties of isotopes

A

different physical properties due to different number of neutrons

same chemical properties as. same number of electrons

some isotopes are radioactive

42
Q

what is relative atomic mass

A

the average value that takes into account the abundance of isotopes for that element

43
Q

what is the relative atomic mass equation

A

(mass number of isotope 1 x percentage abundance of isotope 1) + (mass number of isotope 2 x percentage abundance of isotope 2)
/
100

44
Q

how are elements arranged in the modern periodic table?

A

order of atomic number
elements with similar properties are in groups

45
Q

how do elements in each group have similar properties?

A

same amount of electrons in their outer shell

46
Q

which year did johann obereiner discover his periodic table

A

1817

47
Q

what did johann obereiner discover about the periodic table

A

groups of three elements
appearance and reactions are similar
RAM of middle element close to ram of other 2 elements in the triad
(atomic mass is important in grouping )

48
Q

which year did john newlands discover his periodic table

A

1864

49
Q

how did john newlands arrange his periodic table

A

known elements in order of atomic mass
law of octaves - each element similar properties to the one 8 along
properties repeating but oxygen and iron in the same group was not accepted

50
Q

which year did dimitri mendeleev discover his periodic table

A

1869

51
Q

how was mendeleev periodic table arranged

A

order of atomic mass
left gaps for undiscovered elements
broke his rules - switched tellurium and iodine due to having similar properties to the other group
correctly predicted properties of undiscovered elements

52
Q

which year did henry moseley discover his periodic table

A

1913

53
Q

how is henry moseleys (modern) periodic table arranged

A

grouped by atomic number
knowledge of isotopes explained why order based on atomic weights was not always correct

54
Q

why is the periodic table called a periodic table

A

similar properties occur at regular intervals

55
Q

what are metals

A

elements that react to form positive ions

56
Q

what are non metals

A

elements that do not form positive ions

57
Q

what are group 1 metals

A

alkali metals

58
Q

how does the reactivity change when going down group 1

A

increases

59
Q

how do group1 metals react with water

A

vigorously
create an alkaline solutions and hydrogen

60
Q

how do group 1 metals react with oxygen

A

form an oxide

61
Q

how do group one metals react with chlorine

A

form a white precipitate

62
Q

how does lithium react with oxygen

A

burns with a pink/purple/red flame
white powdery solid

63
Q

how does sodium react with oxygen

A

strong yellow/ orange flame
produces a white solid (sodium oxide)

64
Q

how does potassium react with oxygen

A

large pieces produce vigorous lilac flame then
white solid

smaller ones make solid immediately

65
Q

how does lithium react with water

A

fizzes
gradually disappears
smoke

66
Q

how does sodium react with water

A

fizzes rapidly
melts into a ball
disappears quickly

67
Q

how does potassium react with water

A

lilac flame
sparks
fizzed
disappears fastest

68
Q

how does lithium react with chlorine

A

white powder
settles on sides of container

69
Q

how does sodium react with chlorine

A

bright yellow flame
clouds of white powder settle on sides of container

70
Q

how does potassium react with chlorine

A

more vigorous than with sodium

71
Q

what happens as you go down group 1

A

-more electrons
-more shells
-distance between outer electron and nucleus increases
-more shielding by inner electrons
-easier to lose an electron

72
Q

how does the melting and boiling point change when you go down group 1

A

decreases

73
Q

what are group 7 halogens

A

poisonous non metals
exist as molecules made of pairs of atoms

74
Q

what is tha appearance of fluorine

A

yellow gas

75
Q

what is the appearance of chlorine

A

green gas

76
Q

what is the appearance of bromine

A

red/ orange liquid

77
Q

what is the appearance of iodine

A

purple solid

78
Q

what is the use of fluorine

A

rocket fuel

79
Q

what is the use of chlorine

A

makes drinking water

80
Q

what is the use of bromine

A

clean water of harmful organisms

81
Q

what is the use of iodine

A

used as an antiseptic medicine
turns brown in water

82
Q

what is the trend as you go down group 7

A

relative molecular mass
melting point
boiling point
increase

83
Q

what happens to reactivity as you go past group7

A

decreases

84
Q

why does reactivity decrease for group 7

A

-more electrons
-more shells
-distance between outer electron and nucleus increases
-more shielding by inner electron
-harder to gain an electron

85
Q

what is the displacement in group 7 halogens

A

a more reactive halogen will displace a less reactive halogen from a solution of its salt

86
Q

how many electrons do group 0 noble gases have in their outer shell

A

8

87
Q

what is the trend of reactivity in group 0

A

wont react with anything because they have a full outer shell
don’t form compounds and are monoatomic

88
Q

how does the boiling point of noble gases change

A

increases with increasing relative atomic mass

89
Q

what is the percentage by mass equation

A

% of element = (no of atoms of element x relative atomic mass / relative formula mass of compound) x 100

90
Q

what is the aim of atom economy

A

improving greenness of chemistry
reducing waste made in chemistry industry
saving valuable raw materials
reducing money spent on binning waste from reactions

91
Q

what is atom economy

A

a measure of the amount of starting materials that end up as useful products

92
Q

what does a big percentage of atom economy mean

A

less waste to dispose

93
Q

what is the atom economy equation

A

(relative formula mass of desired product from equation/ sum of
relative formula masses of all reactants from the equation ) x100

94
Q

what are the similarities in chemical properties of group 1 elements compared to transition metals

A

react with non metals to form compounds

95
Q

what are the differences in chemical properties of transition compared to group1 metals

A

g1 - very reactive
-form ions with +1 charge
-react with oxygen quickly
-react with water vigorously
-react with halogens easily

tm- form coloured compounds
-not very reactive
-form ions of different charges
-react with oxygen slowly
-react with water slowly
-react with halogens slowly
-used as catalysts

96
Q

what are the similarities in physical properties of g1 and transition metals

A

good thermal / electrical conductors

97
Q

what are the differences in physical properties of g1 compared to tm

A

tm- high melting point except hg
-malleable
- hard and strong
-high densities

g1- shiny and silver
low melting and boiling points
-low densities
-not as strong
-soft

Chemistry (36 decks)

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