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CHEMISTRY - JAY > Atomic Structure and the Periodic Table > Flashcards

Atomic Structure and the Periodic Table Flashcards

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1
Q

how big is the radius of an atom

A

0.1 nanometers ( 1 x 10(-10))

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2
Q

what charge has the nucleus got?

A

positive

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3
Q

where is most of the mass concentrated in the atom?

A

the nucleus

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4
Q

what determines the size of an atom?

A

the volume of electron orbits

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5
Q

do electrons have mass?

A

they have virtually no mass

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6
Q

whats the overall charge of an atom?

A

neutral (protons and electrons are equal and balanced)

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7
Q

what does the atomic number tell you?

A

number of protons (bottom number)

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8
Q

what does the mass umber tell you?

A

total number of protons and neutrons (top number)

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9
Q

how do you find total number of neutrons?

A

subtract atomic number from the mass number

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10
Q

W hat are isotopes?

A

different forms of the same element, they have the same number of protons but a different number of neutrons, they have the same atomic number but different mass numbers. e.g carbon -12 and carbon-13

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11
Q

what is relative atomic mass?

A

(Ar) an average mass of an element taking into account all its isotopes

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12
Q

what is the formula for Ar

A

sum of (isotope abundance x isotope mass number) / sum of abundance of all isotopes

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13
Q

In a compound formed by metals and non metals, do metal atoms lose or gain electrons?

A

lose electrons, they become positively charged.

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14
Q

In a compound formed by metals and non metals, do non metal atoms lose or gain electrons?

A

gain electrons, the become negatively charged.

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15
Q

Bonding formed by opposite charges reacting is called what?

A

ionic bonding

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16
Q

bonding by sharing electrons is called?

A

covalent bonding

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17
Q

examples of ionic bonding?

A

sodium chloride, magnesium oxide and calcium oxide.

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18
Q

examples of covalent bonding?

A

hydrogen chloride gas, carbon monoxide and water.

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19
Q

what is chromatography?

A

a way of separating different dyes in ink.

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20
Q

how do you carry out chromatography?

A

1- draw a pencil line near the bottom of a sheet of filter paper.
2-add a spot of ink you want to test to the line and place in a beaker of shallow solvent (e.g water)
3- ensure ink isn’t touching solvent as it will dissolve into the liquid.
4- place a lid on container to avoid solvent evaporating.
5- the solvent will carry ink up the filter paper
6- each dye will move up the paper at different rates so the dye will separate out, each dye will form 1 spot,
7-if dyes are insoluble they will stay on the baseline.
8-when the solvent has nearly reached top of the paper, take the paper out to dry

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21
Q

In a chromatography why do you use a pencil

A

because pencil is in soluble.

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22
Q

is water always used as a solvent?

A

no, some compound won’t dissolve in water so other solvents such as ethanol are used.

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23
Q

What does filtration do?

A

sperate insoluble solids from a liquid reaction mixture.

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24
Q

what is purification?

A

solid impurities in the reaction mixture being filtered out of the reaction mixture.

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25
Q

Name two ways to separate soluble solids from solutions.

A

evaporation and crystallisation.

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26
Q

what is evaporation? (separation)

A

heating a solution in a evaporating dish to evaporate the solvent making the solution more concentrated. crystals then form.

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27
Q

what is crystallisation? (separation)

A

heating solution in a evaporating dish to evaporate the solvent to leave a more concentrated solution, when the point of crystallisation is noticeable the dish is removed from heat, the salt then forms crystals and is insoluble. crystals are the filtered out.

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28
Q

examples of when filtration and crystallisation are used?

A

to separate rock salt.

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29
Q

What is rock salt?

A

a mixture of salt and sand (grit)

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30
Q

is rock salt a compound?

A

yes

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31
Q

is rock salt soluble?

A

salt dissolves but sand doesn’t.

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32
Q

How do you separate rock salt?

A

1- Grind rock salt so salt crystals are small (will dissolve easier)
2- put mixture in water, salt will dissolve but sand will not.
3- filter mixture
4- evaporate water to form salt crystals

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33
Q

How can you help salt dissolve?

A

heat the mixture.

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34
Q

What is distillation?

A

separating liquids from mixtures.

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35
Q

what are the types of distillation called?

A

simple and fractional

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36
Q

how do you carry out fractional distillation?

A

1- heat the solution, the liquid with the lowest boiling point will evaporate first.
2-the vapour will then cool and condense in a condenser, you can then collect it.
3- the res of the solution is then left behind in the flask.

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37
Q

what is a condencer?

A

a tube designed to condense gas. the walls are filled with water to cool the gas.

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38
Q

examples of simple distillation

A

to get pure salt from saltwater. the water evaporates first leaving pure salt in the flask.

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39
Q

disadvantages of distillation

A

you can only use it to separate liquids with very different boiling points.

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40
Q

How do you separate liquids with similar boiling points?

A

Fractional distillation.

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41
Q

Give an example of a liquid you could separate by fractional distillation

A

Crude oil

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42
Q

How does fractional distillation work?

A

Liquids have different boiling points so they evaporate at different temperatures. The liquid with the lowest boiling point will evaporate first.

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43
Q

Who described atoms as solid spheres?

A

John Dalton

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44
Q

Who concluded from their experiments that atoms were not solid spheres?

A

J J Thompson

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45
Q

What did J J Thompson’s measurements of charge and mass show about the atom?

A

The presence of electrons

46
Q

Who invented the plum pudding model?

A

J J Thompson

47
Q

What does the plum pudding model show?

A

It shows a ball of positive charge with electrons stuck in it

48
Q

Who showed that the plum pudding model was wrong?

A

Rutherford

49
Q

Describe rutherfords alpha particles scattering experiments.

A

Rutherford fired positively charged alpha particles at an extremely thin sheet of gold.

50
Q

From the Plum Pudding model what did Rutherford expect to see in his scattering experiments?

A

Rutherford expected to see the particles pass straight through the sheet or be slightly deflected bat most.

51
Q

What showed that the Plum Pudding Model couldn’t be right?

A

Some alpha particles were deflected more than expected and some were deflected backwards.

52
Q

What model/idea did rutherford create?

A

The Nuclear Model of the atom

53
Q

Explain the nuclear model of the atom.

A

The nuclear model shows the positively charged nucleus at the centre where most of the pass is concentrated.
a ‘cloud’ of negative electrons surrounding the nucleus

54
Q

Who created a more advanced nuclear model?

A

Bohr.

55
Q

Why did scientists not agree with the theory of a ‘cloud’’ pf negative electrons?

A

The electrons would be attracted to the nucleus causing the atom to collapse.

56
Q

What did Bohr’s model propose?

A

Electrons orbit the nucleus in fixed shells. each shell being a fixed distance from the nucleus.

57
Q

Was Bohr’s theory well supported?

A

yes, It was supported by experiments and helped explain lots of scientific observations at the time.

58
Q

What did further experiments show? (after Bohr’s theory)

A

The existence of Protons.

59
Q

What did Rutherford show about protons?

A

He showed they were smaller particles of the nucleus with the same charge of a hydrogen nucleus.

60
Q

Who provided evidence for neutral particles in the nucleus?

A

James Chadwick

61
Q

What are shells sometimes referred to as?

A

Energy levels.

62
Q

What type of energy level is filled first?

A

Lowest

63
Q

How many electrons are allowed in the first shell?

A

2

64
Q

How many electrons are allowed in the second shell

A

8

65
Q

How many electrons are allowed in the third shell?

A

8

66
Q

In the Early 1800 hundreds what were elements arranged by?

A

Atomic Mass

67
Q

How did Dmitri Mendeleev arrange his periodic table?

A

He put elements in order of atomic mass but he switched the order if the properties meant it should be changed

68
Q

Why did Mendeleev leave gaps in his periodic table?

A

To ensure elements with similar properties stayed in the same groups

69
Q

What did gaps in Mendeleevs periodic table show?

A

The existence of undiscovered elements.

70
Q

What did isotopes show?

A

That mendeleevs periodic table was incorrect and needed to be ordered in atomic mass instead.

71
Q

What are similar properties of Metals?

A
  • They are strong and malleable
  • There great at conducting heat or electricity
  • They have high boiling and melting points
72
Q

What are properties of non-metals?

A
  • dull looking
  • brittle
  • not always solids at room temperature
  • don’t generally conduct electricity
  • lower density
73
Q

Where are transition metals found between?

A

Group 2 and Group 3

74
Q

What are transition metals?

A

They are typical metals

75
Q

What are properties of transition metals?

A
  • They can have more than one ion
  • They are often coloured
  • Transition metal compounds make good catalysts
76
Q

What are group 1 elements known as?

A

Alkali Metals

77
Q

What are the Alkali metals?

A

Lithium, Sodium, Potassium, Rubidium, Caesium and Francium

78
Q

How many electrons are in the outer shell of alkali metals

A

One electron

79
Q

What are alkali metals like?

A

They are all soft and have a low density

80
Q

What are the trends for alkali metals as you go down the group?

A
  • Increasing reactivity (the electron is further away from the nucleus as you go down the group)
  • lower melting and boiling points
  • higher relative atomic mass
81
Q

What ions do group 1 elements form?

A

1+ ions

82
Q

How do alkali metals react with water?

A

They react vigorously to form hydrogen gas and metal hydroxides ( more violent as you go down the group )

83
Q

How do alkali metals react with chlorine?

A

They react vigorously to form white chloride salts, as you go down the group the reaction becomes more vigorous.

84
Q

How do group 1 metals react with oxygen?

A

they react with oxygen to form a metal oxide

85
Q

What oxide does lithium become when reacted with oxygen?

A

lithium oxide.

86
Q

What oxide does sodium become when reacted with oxygen?

A

a mixture of sodium oxide and sodium peroxide.

87
Q

What oxide does potassium become when reacted with oxygen?

A

a mixture of potassium peroxide and potassium superoxide.

88
Q

Whats the difference between alkali metals and transition metals?

A
  • Alkali metals are more reactive then transition metals

- alkali metals are much less dense, strong and hard then the transition metals.

89
Q

What are the group 7 elements also known as?

A

The halogens

90
Q

What are the halogens?

A

Non-metals with coloured vapours.

91
Q

What elements are the halogens?

A

Fluorine, Chlorine, Bromine, iodine and Astatine.

92
Q

What is fluorine?

A

A very reactive poisonous yellow gas.

93
Q

What is chlorine?

A

a fairly reactive, poisonous dense green gas.

94
Q

What is Bromine like

A

A dense, poisonous, red-brown volatile liquid

95
Q

what is iodine?

A

a dark grey crystalline solid or a purple solid.

96
Q

What are the trends of halogens as you go down the group?

A
  • They become less reactive ( its harder to gain an extra electron because its further from the nucleus)
  • increasing boiling and melting points
  • higher relative atomic masses
97
Q

How many electrons do halogens have in their outer shell?

A

7

98
Q

What can halogens form?

A

Molecular compounds

99
Q

How do Halogens share their electrons

A

via covalent bonding with other non-metals

100
Q

What do halogens form with metals?

A

Ionic Bonds

101
Q

Give and example of a ionic bond formed with a halogen .

A

Na(+)Cl(-)

102
Q

What do more reactive halogens displace?

A

less reactive ones

103
Q

What do displacement reactions occur between?

A

A halogen and a salt of a less reactive one.

104
Q

Give an example of halogen displacement.

A

Chlorine can displace bromine and iodine to form an aqueous solution of its salt (iodine and bromine)

105
Q

What are group 0 elements also known as?

A

The noble gases.

106
Q

What are the noble gases?

A

Helium, Neon, Argon, Krypton, xenon and Radon

107
Q

How many electrons are in the outer shell of a noble gas?

A

8 except helium which has two.

108
Q

Noble gases are monatomic gases, What does this mean?

A

they are single atoms not bonds to each other.

109
Q

At room temperature what are noble gases like?

A

colourless gases

110
Q

What are the trends of noble gases as you go down the group?

A
  • Boiling points increase as you go down the group, this is due to greater intermolecular force as more electrons are in the atoms

CHEMISTRY - JAY (3 decks)

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