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Chemistry Overview > C1 The Atom And The Periodic Table > Flashcards

C1 The Atom And The Periodic Table Flashcards

1
Q

John Dalton discovery

Start of 19th centurt

A

Atoms were first described as solid spheres

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2
Q

JJ Thomson

1897

A

Plum pudding model - sphere of positive charge with negative electrons in it

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3
Q

Ernest Rutherford

1909

A

Nuclear model

Alpha scattering experiment

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4
Q

Niels Bohr

Around 1911

A

Electrons in shells orbiting nucleus

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5
Q

James Chadwick

Around 1940

A

Discovered that there are neutrons in the nucleus

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6
Q

Describe the experiment Rutgerford Geiger and Marsden conducted

A

Fired alpha particles at gold foil

Geiger and Marsden’s experiment showed alpha particles rebounded

Led to theory of nuclear atom

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7
Q

Before the discovery of subatomic particles how was the perioidc table arranged

A

In order of their atomic weight

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8
Q

Why were some elements wrong place in the early model of the periodic table

A

Some elements in wrong groups as chemical properties ignored

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9
Q

Law of octaves

A

Every 8th known element was similar

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10
Q

John Newlands peridoic table ordering

A

By mass

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11
Q

What was Dmitri mendeleev order of the periodic table

A

1869 “Father of the periodic table”

Also arranged elements by mass and property, but included empty space for irregular jumps in mass

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12
Q

Why did Mendeleev leave gaps for undiscovered elements in his periodic table?

A

So elements with similar properties could be placed together

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13
Q

What is the periodic table arrangment of atoms order

A

Atomic number

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14
Q

Group 1

A

Alkali metals

Rectivity increases going down group

Increased atomi radii

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15
Q

Reaction for lithium + water

A

Slow reaction

Lithium doesn’t melt

Fizzing can be see and heard as lithium reacts

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16
Q

Lithium + water ———-> Lithium hydroxide + hydrogen

A

2Li(s) + 2H2O(l) ——–> 2LiOH(aq) + H2(g)

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17
Q

Reaction for sodium + water

A

Sodium melts to form a ball that moves around on the surface

Fizzes rapidly before ir disappears

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18
Q

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

A

2Na(s) + 2H2O(l) ———–> 2NaOH(aq) + H2(g)

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19
Q

Reaction for

Potassium + Water → Potassium hydroxide + Hydrogen

A

Reacts violently

Burns with lilac flame

Melts into a shiny ball that rapidly moves around the surface

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20
Q

What does aq stand for in a chemical reaction

A

Aqeous solution

Implies the substance in dissolved in water as the solvent

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21
Q

Redox reaction

A

A chemical reaction that takes place between an oxidizing substance and a reducing substance

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22
Q

Why reactivity of halogens decreases going down the group

A

Going down the group

Outer electron gets further from nucleus

Atoms get larger

Number of shells increase

Nucleus has less attraction for outer electron so increased shell shielding between the nucleus and outer electron

So an electron is gained easily

23
Q

Why reactivity increases going down group 1

A

As go down the group

Atoms get bigger

The outer electron gets further

Attraction between nucleus and last electron gets weaker

So electron more easily lost

24
Q

Why are noble gases unreactive

A

All have full outer shell

All non-metal monatomic elements

25
Q

How do transition metals form coloured compounds

A

Have ions with different charges

26
Q

Compare transition metals to group 1 metals

A

Higher melting points (except mercury)

Higher densities

Stronger

Harder

Less reactive with water and oxygen

27
Q

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

A

High melting point

Hard

Not very reactive

28
Q

Why transition metal oxides added to pottery glazes

A

Colour

29
Q

Atom

A

Smallest part of an element to exist

30
Q

Element

A

Substance made up of only 1 type of atom

31
Q

Metallic

A

Positive ions in a ‘sea’ of delocalised electrons

32
Q

Ionic

A

The strong electrostatic attraction between oppositely charged ions

33
Q

Covalent

A

A shared pair of electrons

34
Q

Why are alloys harder than metals

A

Different sized particles so the layers can not slide across each other as easily

35
Q

How prescence of copper atoms in the alloy results in the alloy being stronger than pure aluminum

A

In pure metals particles same size alloy different sizes

Layers slide over each other easily

In alloys harder to slide over

36
Q

When does ionic conduct electricity

A

When ions are free to move

In molten or solution

37
Q

Describe structure and bonding in sodium chloride

A

Giant lattice structure with strong electrostatic attraction between molecules

38
Q

Features of giant covalent structure

A

Very strong bonds

Very high melting point

Conducts electricity

39
Q

Buckminister fullerene

A

Fullerene with formula C60 carbon atoms joined together by strong covalent bonds

40
Q

Bonds in buckminister fullerene

Medium electrical conductivity

A

Non-bonding electrons and some double C=C covalent bonds

41
Q

What can fullerenes be used for

A

Drug delivery systems in the body, in lubricants and as catalysts

42
Q

Graphene to nanotube

A

High electrical conductivity due to non-bonding electron in its structure similar to graphite

High tensile strength

43
Q

Why diamond has very high melting point

A

Giant covalent lattice

Strong covalent bonds

Lots of heat required to break bonds

44
Q

Why fullerene has low boiling point

A

Weak intermolecular forces of attraction

Little energy required to overcome forces

45
Q

Formula of gallium ion

A

+3
Ga

46
Q

Why discovery of gallium helped mendeleev’s periodic table become accepted

A

Gallium’s properties aligned with Mendeleev’s predictions

47
Q

Gas produced when group 1 elements react with water

A

Hydrogen

48
Q

Type of bonding in sodium

A

Metallic bonding

49
Q

Particles in a sample of neon

A

Ne-20

50
Q

Why sodium oxide has high melting point

A

Strong attractive force between these oppositely charged ions, which require a lot of energy to break

51
Q

Why oxygen described as reduced in reaction sodium and oxygen

A

Oxygen atoms have gained electrons

52
Q

3 differences between nuclear and plum pudding model of atom

A

No empty space plum pudding model

Positive sphere, only nucleus is positive

Neutrons in the nucleus

53
Q

Changes Bohr made to the nuclear model

A

Electrons orbit the nucleus in shells

54
Q

Mendeleev’s reason for reversing order of periodic table

A

Order of atomic number

Chemistry Overview (7 decks)

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