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

C1 The Atom And The Periodic Table Flashcards

(54 cards)

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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

Study These Flashcards
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

Study These Flashcards
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

Study These Flashcards
A

All have full outer shell

All non-metal monatomic elements

25
How do transition metals form coloured compounds
Have ions with different charges
26
Compare transition metals to group 1 metals
Higher melting points (except mercury) Higher densities Stronger Harder Less reactive with water and oxygen
27
2 properties of transition metals that make them suitable for making cutting tools
High melting point Hard Not very reactive
28
Why transition metal oxides added to pottery glazes
Colour
29
Atom
Smallest part of an element to exist
30
Element
Substance made up of only 1 type of atom
31
Metallic
Positive ions in a 'sea’ of delocalised electrons
32
Ionic
The strong electrostatic attraction between oppositely charged ions
33
Covalent
A shared pair of electrons
34
Why are alloys harder than metals
Different sized particles so the layers can not slide across each other as easily
35
How prescence of copper atoms in the alloy results in the alloy being stronger than pure aluminum
In pure metals particles same size alloy different sizes Layers slide over each other easily In alloys harder to slide over
36
When does ionic conduct electricity
When ions are free to move In molten or solution
37
Describe structure and bonding in sodium chloride
Giant lattice structure with strong electrostatic attraction between molecules
38
Features of giant covalent structure
Very strong bonds Very high melting point Conducts electricity
39
Buckminister fullerene
Fullerene with formula C60 carbon atoms joined together by strong covalent bonds
40
Bonds in buckminister fullerene Medium electrical conductivity
Non-bonding electrons and some double C=C covalent bonds
41
What can fullerenes be used for
Drug delivery systems in the body, in lubricants and as catalysts
42
Graphene to nanotube
High electrical conductivity due to non-bonding electron in its structure similar to graphite High tensile strength
43
Why diamond has very high melting point
Giant covalent lattice Strong covalent bonds Lots of heat required to break bonds
44
Why fullerene has low boiling point
Weak intermolecular forces of attraction Little energy required to overcome forces
45
Formula of gallium ion
+3 Ga
46
Why discovery of gallium helped mendeleev's periodic table become accepted
Gallium's properties aligned with Mendeleev's predictions
47
Gas produced when group 1 elements react with water
Hydrogen
48
Type of bonding in sodium
Metallic bonding
49
Particles in a sample of neon
Ne-20
50
Why sodium oxide has high melting point
Strong attractive force between these oppositely charged ions, which require a lot of energy to break
51
Why oxygen described as reduced in reaction sodium and oxygen
Oxygen atoms have gained electrons
52
3 differences between nuclear and plum pudding model of atom
No empty space plum pudding model Positive sphere, only nucleus is positive Neutrons in the nucleus
53
Changes Bohr made to the nuclear model
Electrons orbit the nucleus in shells
54
Mendeleev's reason for reversing order of periodic table
Order of atomic number

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