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atomic structure (seneca) Flashcards

- Elements & compounds - Chemical reactions & equations - mixtures - model of an atom - atom size & number - atomic number - calculations - isotopes - isotopes- calculations - periodic table - noble gases &halogens - alkali metals - transition metals -

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1
Q

what is a Solvent

A

The liquid in which a solid dissolves.

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2
Q

what is a solute

A

dissolved solid

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3
Q

what is a solution

A

A liquid that contains a dissolved solid.

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4
Q

Which technique separates solutions with more than one type of dissolved solid (solute)?

A

chromtography

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5
Q

simple distillation separates …

A

2 liquids with different boiling points

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6
Q

Simple distillation can also separate a

A

solute from a solvent, when the solvent has a lower boiling point than the solute.

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7
Q

Fractional distillation separates

A

lots of liquids with different boiling point

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8
Q

what are the steps of fractional distillation

A

The mixture is slowly heated until the liquid with the lowest boiling point boils and then condenses.
Then we increase temperature slowly to collect (boil then condense) the other fractions.

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9
Q

what are the steps of simple distillation

A

The mixture is heated until the liquid with the lower boiling point starts to boil.
The vapour released passes through a condenser, where the gas cools back into a liquid.

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10
Q

name the main methods of separating liquids

A

Crystallisation
filtration
chromatography
simple distillation
fractional distillation

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11
Q

In ,_____ an English physicist called J. J. Thomson discovered electrons.

A

1897

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12
Q

In ,1897 an English physicist called ———- discovered electrons.

A

J. J. Thomson

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13
Q

In ,1897 an English physicist called J. J. Thomson discovered ——-

A

electrons.

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14
Q

what is thomson’s plum pudding model

A

a ball of positive charge (dough), with negatively charged electrons (currants in pudding) mixed in with the ‘dough’.

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15
Q

In —–, Ernest Rutherford discovered that alpha particles could bounce back off atoms.

A

1909

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16
Q

In 1909, ——— discovered that alpha particles could bounce back off atoms.

A

Ernest Rutherford

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17
Q

In 1909, Ernest Rutherford discovered that ———

A

alpha particles could bounce back off atoms.

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18
Q

In —–, James Chadwick discovered that some particles in the nucleus have no charge at all. He called them neutrons.

A

1932

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19
Q

In 1932, —— discovered that some particles in the nucleus have no charge at all. He called them neutrons.

A

James Chadwick

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20
Q

In 1932, James Chadwick discovered that …

A

some particles in the nucleus have no charge at all. He called them neutrons.

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21
Q

The radius of atoms is

A

aproximately 0.1 nanometres, or 1x10-10 m.

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22
Q

Relative mass =

A

number of protons + number of neutrons

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23
Q

In what environment would the relative mass of an atom change?

A

mass is constant across all environments

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24
Q

The radius of the nucleus is about ——- smaller than the radius of the atom

A

10,000 times

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25
Q

The atomic number is the number —–

A

of protons in the atom

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26
Q

The mass number of an atom (or relative mass) is calculated by …

A

adding the number of protons and neutrons found in a nucleus.

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27
Q

the mass number of an atom is also called

A

relative mass

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28
Q

Protium is a hydrogen atom with

A

1 proton and 0 neutrons.

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29
Q

99.98% of hydrogen atoms are

A

protium.

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30
Q

Protium is used in

A

hydrogen fuel cells and the production of plastics.

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31
Q

Deuterium is a hydrogen atom with

A

1 proton and 1 neutron.

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32
Q

Around 0.02% of hydrogen atoms are

A

deuterium.

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33
Q

deuterium is used in

A

nuclear fusion.

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34
Q

Tritium is a hydrogen atom with

A

1 proton and 2 neutrons.

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35
Q

Tritium is used in

A

thermonuclear fusion weapons.

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36
Q

Tritium is (%) …

A

very rare.

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37
Q

what are isotopes

A

Atoms of the same element that have different numbers of neutrons.

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38
Q

The Σ means

A

sum of

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39
Q

calculate relative atomic masses (Ar) with isotope abundance

A

Σ(isotope abundance x isotope mass number/Σ isotope abundance

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40
Q

Σ(isotope abundance x isotope mass number/Σ isotope abundance
The numerator is

A

‘the sum of the isotope abundance times the isotope mass number’.

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41
Q

Σ(isotope abundance x isotope mass number/Σ isotope abundance
The denominator is

A

‘the sum of all the isotope abundances’.

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42
Q

Electrons fill an atom’s shells in order of

A

increasing energy

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43
Q

The closer a shell is to the nucleus,

A

the lower its energy level, so the first shell that is filled is the closest to the nucleus

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44
Q

Electron configuration tells us how

A

an atom’s electrons are organised.

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45
Q

in the calculation Σ(isotope abundance x isotope mass number/Σ isotope abundance, Σ isotope abundance will add to …

A

100 %

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45
Q

relative atomic mass= Σ
​

A

(isotope abundance×isotope mass number)/100

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46
Q

what is Relative atomic mass (1)

A

The relative atomic masses (Ar) of elements are calculated using the average mass of all of the isotopes of an element.

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47
Q

the horizontal rows of the periodic table are called

A

periods.

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48
Q

Elements in the same column have the ——– in their outer shell (the highest energy level).

A

same number of electrons

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49
Q

Because all elements in a column have the same number of electrons in their outer shell,

A

they have similar chemical properties.
This means they will all react in similar ways.

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50
Q

——— was the first chemist to devise a periodic table.

A

John Newlands

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51
Q

Newlands’ periodic table was ordered by …

A

the mass of the element.

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52
Q

the Newlands’ table was incomplete, and some elements were

A

placed in inappropriate groups.

53
Q

Dmitri Mendeleev recognised that there may be

A

undiscovered elements

54
Q

—— added gaps to Newlands’ table to account for undiscovered elements.

A

Mendeleev

55
Q

Mendeleev even predicted the

A

properties and masses of these undiscovered elements

56
Q

The discovery of protons and isotopes has shown that Mendeleev ordered elements exactly by

A

relative atomic mass.

57
Q

Metals have —- melting and boiling points.

A

high

58
Q

When metals react, they

A

lose 1 or more of these negatively charged electrons to form positively charged ions

59
Q

Metals are —- conductors of heat and electricity.

A

good

60
Q

Metals are ——————- at room temperature.

A

all solids (except for mercury)

61
Q

When non-metals react, they either:

A

Gain electrons to form negatively charged ions.
Or share electrons to form neutral molecules

62
Q

Non-metals are found on the right of the periodic table because they

A

have many electrons in their outer shell.

63
Q

non-metals have —- melting and boiling points than metals

A

lower

64
Q

Non-metals are often found as

A

gases.

65
Q

Non-metals generally —– heat or electricity.

A

do NOT conduct

66
Q

The elements in Group 0 are

A

unreactive because they have a full outer electron shell. They do NOT gain or lose electrons to fill up this shell as it is already full.

67
Q

Noble gases can be used in light bulbs because

A

they will NOT react with the hot metal filament.

68
Q

Because noble gases are unreactive, they exist as

A

single atoms (monatomic) instead of forming molecules.

69
Q

The noble gases have — boiling points.

A

low

70
Q

the noble gases’ boiling points do …..
This is because…

A
  • increase as you move down the periodic table.
  • the relative atomic mass increases lower down the periodic table.
71
Q

The noble gases (in group 0) have —- densities

A

low

72
Q

the noble gases’ densities do
this is because …
This — density makes them useful….

A
  • increase as you move down the periodic table because of their increasing relative atomic mass.
  • This low density makes them useful in balloons.
73
Q

nobles gases are (meaning unreactive)…

A

inert

74
Q

what are properties of noble gases(5)

A

inert
colourless
monatomic
low boiling points
low density

75
Q

Halogens are in group – and so have …

A

7
7 electrons in their outer shell.

76
Q

In their elemental form, halogens share electrons to make

A

diatomic molecules (molecules made of pairs of atoms)

77
Q

When a metal atom transfers its outer electron to a non-metal atom (like a group 7 atom),——— are formed.

A

salts

78
Q

As you move down the group, the halogens decrease in reactivity. This is because:

A

The atoms gain more electron shells.
So, the distance between the outer electron shell and the nucleus increases.
So, the attraction between the nucleus and the electron (to be gained from another element) decreases.

79
Q

As you move down the group, the halogens —— in reactivity

A

decrease

80
Q

give two examples of halogens that fluorine displace from a compound?

A

chlorine and bromine

81
Q

Why do halogens become less reactive as you go down the group?

A

the electron gained from another element is further from the nucleus

82
Q

Lithium is the —— reactive of the alkali metals

A

least

83
Q

Lithium burns with a ——- flame when it reacts with oxygen.

A

crimson

84
Q

Lithium —– on the surface of water and will release ——-

A

floats
bubbles of hydrogen gas (it effervesces).

85
Q

Sodium is —– reactive than lithium because —–
This is because it is

A

more
its outer electron is less strongly attracted to the positively charged nucleus.
a greater distance from the positive charge of the atom’s nucleus.

86
Q

The metal —- on the surface of water, which releases —.
The sodium moves

A
  • floats
  • enough heat to melt the sodium
  • quickly across the surface of the water.
87
Q

Sodium burns with a ——
flame when it reacts with oxygen.

A

yellow/orange

88
Q

Potassium is more reactive than —–because —–.

A

lithium and sodium
its outer electron is least strongly attracted to the nucleus

89
Q

The potassium floats on the surface of water, and

A

has a similar, but more vigorous, reaction compared with sodium

90
Q

Potassium burns with a —- flame when it reacts with oxygen.

A

lilac

91
Q

the elements found in group 1 are called

A

alkali metals

92
Q

when alkali metals react with oxygen, they…

A

Rapidly turns from silvery shiny to dull as a metal oxide (e.g. potassium oxide) is produced.

93
Q

when alkali metals react with chloride, a…

A

A metal chloride is formed (e.g. sodium chloride), which dissolves in water to give a colourless solution.

94
Q

when alkali metals react with water they…

A

The metal floats on the surface and melts to create a metal hydroxide (e.g. lithium hydroxide).
When they react with water, the energy released is enough to melt the metal.

95
Q

As you move down Group 1 of the periodic table, the reactions of alkali metals become

A

quicker and more vigorous

96
Q

As you move down Group 1 of the periodic table, the reactions of alkali metals become quicker and more vigorous. Explain

A

The number of electron shells increases meaning there is a greater distance between the outer electron and the nucleus.
The greater the distance between the outer electron and the nucleus, the weaker the attraction between them.
The weaker the attraction between the outer electron and the nucleus, the easier it is for the outer electron to be lost.

97
Q

The transition metals are found in the ——- of the periodic table.

A

middle

98
Q

Transition metals are —–reactive than alkali metals.
E.g.

A

less
Iron takes weeks to rust when in contact with oxygen and water, whereas sodium does this in a few seconds.

99
Q

Transition metals have —- melting points than alkali metals.
E.g.

A

higher
Iron’s melting point is 1,583°C, whereas sodium’s is about 98°C.

100
Q

—- melting points make transition metals useful for …

A

High
cooking equipment.

101
Q

Transition metals are ———— than alkali metals.

A

stronger and harder

102
Q

Transition metals have more mass for the —- volume than alkali metals.
The —- density makes transition metals useful in —-

A

same
high
construction.

103
Q

form the iron ions with different positive charges

A

Fe2+, Fe3+

104
Q

form the copper ions with different positive charges

A

Cu+, Cu2+

105
Q

Copper(I) sulfate is (colour)

A

white

106
Q

copper(II) sulfate is (colour)

A

blue.

107
Q

Iron (Fe) is the catalyst used in the —-, which results in the production of —-

A
  • Haber process
  • ammonia.
108
Q

Platinum (Pt) and rhodium (Rh) are used as the catalyst for

A

catalytic converters in cars.

109
Q

Used in catalytic converters in cars.

A

Platinum
and rhodium

110
Q

Relative to the alkali metals, transition metals have: 1. melting points,2. density and 3. reactivity.

A
  1. higher
  2. higher
  3. lower
111
Q

Transition metals have special properties of (3)

A
  • are often used as catalysts
  • can form colourful compounds
  • can form positive ions with different positive charges
112
Q

Which group of elements form DIATOMIC MOLECULES and become LESS REACTIVE as you move down the group?

A

group 7

113
Q

what are properties of metals?

A

high melting and boiling points
good conductors
they lose electrons when they react

114
Q

What is the relative atomic mass?

A

The relative atomic mass is the average mass of an element, weighted according to the abundance of its isotopes, on a scale where carbon-12 has a mass of 12.

115
Q

Why is only half the water evaporated initially in crystallisation for hydrated copper sulfate crystals?

A

The aim of the experiment is to gain hydrated copper sulfate crystals. This means that the crystal itself should have some water in it.
If the solution is boiled dry, even the copper sulfate will lose its water and become dry, i.e. anhydrous copper sulfate.
Anhydrous copper sulfate is a white solid while hydrated copper sulfate is blue.
If a question asks for a hydrated salt, make sure to mention that you do not boil off all the water. Instead, let half the solution evaporate by itself.

116
Q

what is a ion?

A

a charged atom either negative or positive

117
Q

What was the name of the atomic model devised by J.J. Thomson?

A

plum pudding model

118
Q

Rutherford’s atomic model was called the —–.

A

nuclear model

119
Q

What conclusions did Ernest Rutherford draw from his discovery that alpha particles could bounce back off atoms?

A

an atoms mass is concentrated in its centre
the nucleus contains positively charged particles

120
Q

Calcium carbonate reacts with hydrochloric acid to form calcium chloride, carbon dioxide, and water. what is the balanced equation for this reaction?

A

CaCO3+2HCI –> CaCl2+CO2+H20

121
Q

Lime water before reacting with carbon dioxide is …

A

Colourless (NOT CLEAR)

122
Q

Acid + oxides ->

A

Salt + water

123
Q

Acid + hydroxides ->

A

Salt + water

124
Q

Acid + carbonates ->

A

Salt + water + carbon dioxide

125
Q

what are monatomic atoms?

A

A molecule composed of just one atom, and lacking any covalent bonds

126
Q

Atomic number=

A

Number of protons

127
Q

What are properties of metals (5)?

A
  • Shiny
  • Mostly solid
  • Dense and strong
  • Malleable
  • Good heat and
    electrical conductors
128
Q

What are properties of non-metals (5)?

A
  • Dull
  • Low density
  • Weak
  • Brittle
  • Poor heat and
    electrical conductors
129
Q

What does sonorous mean?

A

Makes a ringing sound when hit.

science chemistry (18 decks)

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