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Chemistry > C2 Periodic Table > Flashcards

C2 Periodic Table Flashcards

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1
Q

Why ordering of elements changed overtime

A

New elements were being found and scientists needed to rearrange them by relative atomic mass

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2
Q

How the electronic structure of metals and non-metals are different

A

Atoms of metal give away electrons to form positive ions

Atoms of non-metal gain electrons to form negative ions

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3
Q

How the electronic structure of metals and non-metals affects their reactivity

A

If an atom has more electrons than protons its reactivity increases

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4
Q

How electronic structure is linked to the periodic table

A

The number of electrons in outermost shell depends on the group number the element is in

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5
Q

How to use the periodic table to predict reactivity of elements

A

For metals reactiviy increases down a group

Reactivity decreases moving left to right along a period

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6
Q

Why are noble gases unreactive

A

The atoms of noble gases already have complete outer shells so they have no tendency to lose, gain or share electrons

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7
Q

How to predict which ions are stable

A

How easily an element can achieve a full outer electron shell

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8
Q

Properties of group 1 metals

A

Soft

Reactive

Low melting points

Good conductors of heat and electricity

Low density

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9
Q

Why elements in group 1 react similarly

A

They all have 1 electron in their outer shell

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10
Q

Why do the first 3 elements of group 1 float on water

A

Less dense than water

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11
Q

Equation for group 1 metals react with water

A

2X(s) + 2H2O(s) —> 2XOH(aq) + H2(g)

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12
Q

How you can show that hydrogen and metal hydroxides are made when Group 1 metals react with water

A

Hydroxides dissolve in water to form alkaline solutions

They are purple showing they are strongly alkaline

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13
Q

How Group 1 metals are stored and the safety precautions used when dealing with them

A

Stored in mineral oil or kerosene

Do not expse to air or water

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14
Q

How to recognise a halogen displacement reaction

A

Reaction mixture turns darker and iodine solution forms

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15
Q

Why elements in group 7 react similarly

A

Same number of electrons in outer shell

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16
Q

Main properties of halogens

A

Form negative anions

More dense as go down group

Poor conductors of heat and electricity

Brittle

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17
Q

How to complete a halogen displacement reaction

A

2 drops potassium chloride to each 3 dimples in column 1 of tile

2 drops potassium bromide solution to each of 3 dimples in column 2

2 drops potassium iodide solution to each of 3 dimples in column 3

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18
Q

What happens in halogen displacement reaction

A

The more reactive halogen atoms oxidise the less reactive halide ions

causing halide ions to lose electrons and form halogen atoms

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19
Q

Trend in reactivity group 1 metals

A

Increases as you go down the group

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20
Q

Reactivity of group 7

A

Decreases as go down the group

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21
Q

Why group 1 reactivity increases as go down the group

A

As go down the group

Atoms get larger

Outer electron gets further from nucleus

Attraction between nucleus and outer electron gets weaker so electron is easily more lost

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22
Q

Why group 7 reactivity decreases as go down the group

A

As you go down the group

Atomic mass of halogens increases

Increases in electron shells

Atoms get larger as go down the group therefore attraction of outer electron to nucleus decreases as you go down group 7

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23
Q

Trend in group 1 boiling point

A

Decreases

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24
Q

Why group 1 boiling point decreases as go down the group

A

As go down the group there are more protons, electrons, neutrons and energy levels to the atoms

Atoms get larger

As atom increase in size attractive forces decrease since internuclear distance increases

This leads to lower boiling and melting temperatures

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25
Q

Trend in group 7 boiling points

A

Increases

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26
Q

Why trend in boiling point increases as you go down group 7

A

Atoms increase in size as they gain electron shells

Intermolecular forces are stronger

More energy required to break these forces
so higher boiling and melting points as go down the group

Halogens have covalent bonding

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27
Q

How to use nuclear model to explain how the outer electrons experience different levels of attraction to the nucleus

A

Higher effective nuclear charge causes greater attractions to electrons

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28
Q

Properties of transition metals

A

Hard

Strong

High melting boiling points

Good conductors of heat and electricity

Dense

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29
Q

Use of transition metals

A

Iron used to make steel used to build buildings

Copper used for coins

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30
Q

Why mercury is not a typical transition element

A

Neither the atom or its cations posses an incomplete d-subshell

31
Q

Why Group 1 metals have different properties compared to transition metals

A

Transition metals react slowly or not at all

32
Q

Why can we be confident there are no missing elements in the first 10 elements of periodic table

A

Element is identified with the number of protons in nucleus

Any atom with 6 protons is carbon it cannot be anything else

33
Q

Patterns in periodic table

A

Atomic radius

Electronegativity

Metallic character

34
Q

Why elements in same group react the same way

A

Similar number of valence electrons

35
Q

Metal and non-metal ions

A

Metal atoms lose electrons to form positive ions

Non-metal atoms gain electrons to form negative ions

36
Q

What happens when group 1 metals react with water

A

Reacts vigorously to produce hydrogen gas and metal hydroxides

37
Q

What happens when group 1 metals react with chlorine

A

React vigorously to form white metal chloride salts

38
Q

What happens when group 1 metals react with oxygen

A

They react with oxygen to form a metal oxide

Lithium reacts with oxygen to form lithium oxide (Li2O)

39
Q

2 differences between the physical properties of group 1 metals and transition metals

A

Group 1 metals are malleable and ductile

40
Q

2 differences between the chemical properties of group 1 metals and transition metals

A

Higher melting point

Less reactive

41
Q

Similarities between the properties of group 1 metals and transition metals

A

Good conductors of heat and electricity

Easily oxidised to form cations

React with water

42
Q

Colour of fluorine, chlorine poisonous gases

A

Fluroine - yellow

Chlorine - dense green

43
Q

Colour of bromine (poisonous) and iodine

A

Bromine - Red-brown liquid

Iodine - dark grey crystalline solid or purple vapour

44
Q

What happens to relative atomic masses of halogens as you go down the group

A

Higher relative atomic masses

45
Q

Structures of compounds formed

A

Ionic

46
Q

What do group 0 elements exist as

A

Monotomic gases

47
Q

Monatomic gases

A

Single atoms not bonded to each other

48
Q

What state are group 0 at room temperature

A

Colourless gases

49
Q

Why does boiling point increase as you go down group 0

A

Due to an increase in number of electrons in each atom leading to greater intermolecular forces

50
Q

Trend reactivity in group 0

A

Noble gases are unreactive

51
Q

Formula sodium carbonate

A

Na2CO3

52
Q

How were elements arranged periodic table early 1800s

A

Atomic weight

53
Q

Which were the 2 obvious ways to categorise elements

A

Physical and chemical properties

Atomic weight

54
Q

Where does the name periodic table come from

A

The periodic table got its name from how elements are arranged in rows called periods

55
Q

Why were early periodic tables not complete and some elements placed in wrong group

A

Because elements were placed in order of atomic weight

56
Q

1869 what order did Dmitri Mendeleev order elements

A

Order of atomic weight

57
Q

1869 what order did Dmitri Mendeleev order elements

A

Order of atomic weight

58
Q

Why did Dmitri Mendleev leave gaps in periodic table 1869

A

To make sure elements with similar properties stayed in same groups

Some of these gaps indicated existence of undiscovered elements elements and allowed Mendeleev to predict what their properties might be

59
Q

Why was discovery of isotopes in the 20th century important for Mendeleev

A

It confirmed Mendeleev was correct to not place elements in a strict order of atomic weight but to also take account of their properties

60
Q

John Newlands 1864

A

Noticed periodicity based on elemental mass and sorted elements by mass 1864

61
Q

Law of octaves

A

Every 8th known element was similar

62
Q

Which properties of elements did Dmitri Medeleev predict before they were discovered

A

Scandium

Gallium

Technetium

Germanium

63
Q

Who was Dmitri often referred to as

A

“Father of the periodic table”

64
Q

What is the periodic table arranged in

A

Order of atomic number

65
Q

Word equation of group 1 elements react with water

A

Lithium + water ———–> Lithium hydroxide + hydrogen

Sodium + water ———–> sodium hydroxide + hydrogen

66
Q

Observations when lithium reacts with water

A

Slow reaction

Lithium doesn’t melt

Fizzing

67
Q

Observations when sodium reacts with water

A

Sodium melts

Hydrogen released catches fire and causes the ball to dash across surface

68
Q

Observations when potassium reacts with water

A

Burns with lilac coloured flame

Melts into shiny ball that dashes around surface

69
Q

State of bromine at 0° and 100°

A

0° - liquid

100° - gas

70
Q

Colour change when chlorine reacts with sodium bromide

A

Colour at start - colourless

Colour at end - brown

71
Q

2 properties of transition metals that make them suitable for cutting tools

A

High melting point (can withstand high temperatures)

Hard

72
Q

Why transition metal oxides are added to pottery glazes

A

Colour

73
Q

79
Br
35

Number of neutrons?

A

35 = number of protons

79 - 35 = 44 = number of neutrons

Chemistry (10 decks)

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