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Alex M Science > Atomic Structure And The Periodic Table (paper 1) > Flashcards

Atomic Structure And The Periodic Table (paper 1) Flashcards

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1
Q

What are alkali metals?

A

The elements in Group 1 of the periodic table.

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2
Q

What is an atom?

A

The smallest part of an element that can exist. All substances are made up of atoms.

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3
Q

What is the atomic nucleus?

A

Positively charged object composed of protons and neutrons at the centre of every atom with one or more electrons orbiting it.

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4
Q

What is the atomic number?

A

The number of protons in the nucleus.

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5
Q

What is chromatography?

A

A separation technique used to separate a mixture of chemicals by distributing the components between two phases.

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6
Q

What is a compound?

A

A substance made up of two or more types of atoms chemically combined together.

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7
Q

What is crystallisation?

A

A separation technique used to produce solid crystals from a solution by evaporating the solvent.

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8
Q

What is displacement in chemistry?

A

A chemical reaction in which a more reactive element displaces a less reactive element from its compound.

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9
Q

What is an electron?

A

Negatively charged subatomic particle which orbit the nucleus at various energy levels. Very small relative mass (negligible).

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10
Q

What is an electron shell?

A

Different energy levels in atoms occupied by electrons.

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11
Q

What is an element?

A

A substance made up of only one type of atom.

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12
Q

What is filtration?

A

A separation technique used to separate solids from liquids.

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13
Q

What is fractional distillation?

A

A method of separating a mixture of substances according to their different boiling points.

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14
Q

What is a group in the periodic table?

A

The columns of the periodic table represent different groups of elements. Elements with similar properties are in the same group.

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15
Q

What are halogens?

A

The elements in Group 7 of the periodic table.

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16
Q

What is an ion?

A

An atom or molecule with an electric charge due to the loss or gain of electrons.

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17
Q

What is an isotope?

A

Atoms of the same element with the same number of protons but a different number of neutrons.

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18
Q

What is the mass number?

A

The total number of protons and neutrons in the nucleus.

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19
Q

What are metals?

A

Elements that react to form positive ions. Found to the left and towards the bottom of the periodic table.

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20
Q

What is a mixture?

A

A mixture consists of two or more elements or compounds not chemically combined together.

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21
Q

What is a neutron?

A

Neutral subatomic particle present in the nucleus of the atom. Relative mass of 1.

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22
Q

What are noble gases?

A

The elements in Group 0 of the periodic table.

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23
Q

What are non-metals?

A

Elements that react to form negative ions. Found towards the right and top of the periodic table.

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24
Q

What is the nuclear model?

A

The nuclear atomic model stated that the mass was concentrated at the centre of the atom and that the nucleus was charged.

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25
What is the periodic table?
Table of elements arranged in order of atomic number and such that elements with similar properties are in the same column (group).
26
What is the plum pudding model?
Atomic model devised after the discovery of the electron. The model suggests the atom is a ball of positive charge with negative electrons scattered through it.
27
What is a proton?
Positively charged subatomic particle present in the nucleus of the atom. Relative mass of 1.
28
What is relative atomic mass?
An average value that takes account of the abundance of the isotopes of the element.
29
What is simple distillation?
A procedure by which two liquids with different boiling points can be separated.
30
What are transition metals?
The collection of metallic elements in the middle of the periodic table.
31
How did john newlands order the periodic table
In order of atomic WEIGHT
32
How did Mendeleev order the periodic table
In order of atomic mass But later realised they didn’t have similar chemical properties Left spaces in it for undiscovered elements
33
Why is the periodic table called that
Similar properties occur at regular intervals
34
What are the rows and columns called in the periodic table
Periods (horizontal) and groups (perpendicular)
35
What is group 1 and what are their properties
Alkali metals Physical Properties: • Soft (can be cut with a knife; softness increases down the group). • Low density – lithium, sodium, and potassium float on water. • Shiny when freshly cut, but quickly tarnish in air due to oxidation. • Good conductors of electricity. • Low melting and boiling points (decrease down the group). Chemical Properties: • React with oxygen to form metal oxides • React with water to form a metal hydroxide and hydrogen gas Trends Down the Group (Top to Bottom): • Reactivity increases – outer electron is more easily lost. • Softness increases. • Melting and boiling points decrease. • Density increases (but not always linearly).
36
Why does reactivity increase going down the group
• Outer electron is further from the nucleus. • Increased shielding by inner electron shells. • Weaker electrostatic attraction between nucleus and outer electron. • So, outer electron is lost more easily.
37
How does lithium react with oxygen?
It burns with a strongly red-tinged flame and makes a white solid.
38
How does lithium react with water?
It fizzes steadily and disappears gradually.
39
How does lithium react with chlorine?
A white powder is produced and settles on the sides of the container.
40
How does sodium react with oxygen?
It burns with a strong orange flame and makes a white solid.
41
How does sodium react with water?
It fizzes rapidly, melts into a ball, and disappears quickly.
42
How does sodium react with chlorine?
It burns with a bright yellow flame, making clouds of white powder that settle on the sides of the container.
43
How does potassium react with oxygen?
Large pieces produce a lilac flame; small ones turn into a solid immediately.
44
How does potassium react with water?
It ignites with sparks and a lilac flame, and disappears very quickly.
45
How does potassium react with chlorine?
The reaction is even more vigorous than with sodium.
46
How many electrons do noble gases have in their outer shell?
They have 8 electrons (except helium, which has 2).
47
Why are noble gases unreactive?
They have a full outer shell of electrons, so they don’t easily form molecules.
48
What happens to the boiling point of noble gases as you go down the group?
The boiling points increase with increasing relative atomic mass.
49
How many electrons do halogens have in their outer shell?
7 electrons.
50
Do halogens exist as single atoms or molecules?
They exist as molecules made of pairs of atoms (e.g., Cl₂).
51
How do halogens react with metals?
They form ionic compounds where the halide ion carries a -1 charge.
52
How do halogens react with non-metals?
They form covalent compounds by sharing a pair of electrons.
53
What happens to the melting and boiling points as you go down Group 7?
They increase.
54
What happens to reactivity as you go down Group 7?
Reactivity decreases.
55
Why does reactivity decrease down Group 7?
Because: - Halogens gain an electron to fill their outer shell. - More electron shells = more shielding. - So atoms attract electrons less easily.
56
What is displacement in halogens?
A more reactive halogen can replace a less reactive one in a solution of its salt.
57
Example of displacement reaction:
Chlorine + Potassium Bromide → Potassium Chloride + Bromine
58
What is an element?
A substance made of only one type of atom.
59
What is an isotope?
Atoms of the same element with the same number of protons but a different number of neutrons.
60
Where are electrons found?
In energy levels (shells) around the nucleus.
61
What is the maximum number of electrons in the first three shells?
1st shell: 2 2nd shell: 8 3rd shell: 8
62
How do you work out an atom’s electronic configuration?
Use the atomic number to count the electrons, then fill the shells in order.
63
What did Dalton think atoms were like?
Solid spheres.
64
What did the plum pudding model suggest?
A ball of positive charge with electrons stuck in it.
65
What did Rutherford’s gold foil experiment show?
That atoms have a tiny, dense, positively charged nucleus.
66
What did Bohr suggest?
Electrons move in fixed orbits (energy levels) around the nucleus.
67
Why was the neutron discovered later?
It has no charge, so it was harder to detect.
68
What is the relative mass and charge of a proton?
Mass: 1 Charge: +1
69
What is the relative mass and charge of a neutron?
Mass: 1 Charge: 0 (neutral)
70
What is the relative mass and charge of an electron?
Mass: Very small (almost 0 – about 1/1836) Charge: -1
71
Which subatomic particle decides the atomic number of an element?
The proton.
72
Why do atoms have no overall charge?
Because the number of protons equals the number of electrons, so the charges cancel out.
73
What is an atom?
The smallest particle of an element that still has its properties.
74
What is the atomic number?
The number of protons in an atom.
75
What is the mass number?
The number of protons + neutrons.
76
What is a mixture?
A combination of two or more substances that are not chemically joined.
77
What is a compound?
A substance made from two or more elements chemically bonded together in fixed proportions.
78
Can mixtures be separated easily?
Yes, because the substances are not chemically bonded.
79
Can compounds be separated easily?
No, you need a chemical reaction to separate them.
80
Do mixtures have fixed compositions?
No – the amounts of substances can vary.
81
Do compounds have fixed compositions?
Yes – they have a set ratio of atoms.
82
How do you separate an insoluble solid from a liquid?
Use filtration.
83
How do you separate a soluble solid from a liquid (e.g., salt from water)?
Use evaporation or crystallisation.
84
How do you separate two liquids with different boiling points?
Use simple distillation (for big difference) or fractional distillation (for similar boiling points).
85
How do you separate the different dyes in ink?
Use paper chromatography.
86
What does chromatography show?
It shows the different substances in a mixture based on how far they travel on the paper.
87
What is the mobile phase in chromatography?
The solvent that moves through the paper.
88
What is the stationary phase in chromatography?
The paper the solvent moves through.

Alex M Science (8 decks)

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