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GCSE Chemistry > Atomic Structure and the Periodic Table > Flashcards

Atomic Structure and the Periodic Table Flashcards

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1
Q

Structure of the Nucleus

A
  • In the centre of the atom
  • Contains protons and neutrons
  • Positively charged because of protons
  • Has a radius of 1x10-14
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2
Q

Electrons

A
  • Orbit the nucleus in shells
  • Negatively charged
  • Volume of orbit determines size of the atom
  • Have a very small mass
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3
Q

Proton Relative Mass and Charge

A
  • Relative Mass: 1
  • Charge: +1
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4
Q

Neutron Relative Mass and Charge

A
  • Relative Mass: 1
  • Charge: 0
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5
Q

Electron Relative Mass and Charge

A
  • Relative Mass: Very Small
  • Charge: -1
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6
Q

Why is the overall charge of an atom 0?

A

There are an equal amount of protons and electrons in an atom so the charge cancels out

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7
Q

Relative Atomic Mass Formula

A

Total mass of atoms/Total number of atoms

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8
Q

Top and Bottom Numbers on Nuclear Symbol

A
  • Top: Mass Number
  • Bottom: Atomic Number/Proton Number
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9
Q

Number of Neutrons Calculation

A

Mass Number - Atomic Number

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10
Q

Solute

A

A substance that is being dissolved in a solvent

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11
Q

Solvent

A

The liquid that the solute dissolves in

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12
Q

Solution

A

A mixture made when a solute dissolves into a solvent.

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13
Q

Simple Distillation

A

Used to separate a liquid from a solution

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14
Q

Simple Distillation Method

A
  • Heat flask using a bunsen burner so the liquid that is being separated evaporates
  • The vapour of said liquid rises to the top of the flask and passes through the condenser
  • The cold water in the condenser causes the vapour to cool and condense
  • The liquid runs down the pipe and is collected in a beaker
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15
Q

Fractional Distillation

A

Used to separate mixtures of liquids with different boiling points

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16
Q

Fractional Distillation Method

A
  • Heat flask using a bunsen burner so the liquid with the lowest boiling point condenses first
  • The vapour rises through a column that is hotter at the bottom and cooler at the top
  • It rises up the fractioning column, passes through the condenser and condenses
  • Collect the condensed liquid
  • You are left with the other liquid in the flask
17
Q

Newlands Periodic Table

A
  • Ordered by atomic weight and maintained this order
  • Every 8 elements had similar properties
  • Didn’t work as it forced Newlands to group elements that didn’t have similar chemical properties
  • Wasn’t accepted by other scientists
18
Q

Mendeleev’s Periodic Table (The table we use to this day)

A
  • Ordered elements by atomic weight
  • Left gaps for undiscovered elements
  • Swapped the order of some elements based on if their properties matched better elsewhere
  • Elements in groups had similar chemical properties
  • Accepted by other scientists when newly discovered elements were found to fit Mendeleev’s system
19
Q

Why do metals form positive ions?

A
  • They don’t have many electrons in their outer shells
  • The outer electron can be lost more easily as it would require less energy
20
Q

Why does reactivity increase down metal groups?

A
  • Elements further down the table have more shells
  • The outer shell would be further from the nucleus so the attraction between the 2 is weaker
  • The electron is more easily lost
21
Q

Non Metals

A

Form either no ions or negative ions

22
Q

Metal Properties

A
  • High melting and boiling points so are solids at room temperature
  • Good conductors of heat and electricity
  • Lustrous (shiny)
  • Malleable
  • Sonorous
  • Have high densities
23
Q

Non Metal Properties

A
  • Poor conductors of heat and electricity
  • Appear dull
  • Weak and brittle
  • Low melting and boiling points so liquids and gases at room temperature
  • Not sonorous
  • Low densities
24
Q

Transition Metals

A
  • Can form more than 1 type of ion
  • Form coloured ions
  • Melting points and densities are higher than group 1 metals
  • Stronger and harder than group 1 metals
  • Shiny when freshly cut
25
Q

Group 1 Metal Properties

A
  • Reactive, soft metals
  • Alkali metals
  • Low density
  • More reactive than transition metals
  • React vigorously with water, oxygen and group 7 elements
26
Q

Group 1 Trends

A
  • Reactivity increases down the group
  • Melting and boiling point decrease down the group
  • Relative atomic mass increases down the group
27
Q

Group 1 Reactions

A
  • Group 1 + water –> Metal Hydroxide + Hydrogen
  • Group 1 + Chloride –> Metal Chloride + Salt
  • Group 1 + Oxygen –> Metal Oxide
28
Q

Group 7 Properties

A
  • Non metals
  • All halogens are diatomic molecules
  • At room temperature, fluorine is a pale yellow gas, chlorine is a pale green gas, bromine is an orange liquid and iodine is a grey solid
29
Q

Group 7 Trends

A
  • Relative atomic mass increases down the group
  • Melting and boiling points increase down the group
  • Reactivity decreases down the group
30
Q

Group 0

A
  • Have full outer shells so they are unreactive
  • Exist as single atoms
  • Non-flammable
  • Boiling point increases down the group
31
Q

What is the limitation of a dot and cross diagram?

A

It doesn’t show how the atoms are arranged in space

32
Q

What are the limitations of a ball and stick diagram?

A
  • Not to scale
  • Doesn’t give information about the forces pf attraction of the movement of electrons to form the ions

GCSE Chemistry (7 decks)

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