1. Chemistry Spaced Learning Triple

2. C1
This atom is from an element in group 4.
The mass of this atom is

3. Li 3 7 C1 The atomic number tells you how many electrons the atom has.
The mass number tells you how many particles are in the nucleus of the atom.
Particle
Location
Relative Mass
Relative Charge
Proton
Nucleus 1 +1
Neutron
Electron
Shells -1

4. Atoms and Isotopes
Mass Number
Atomic Number
An isotope of an element has the same number of electrons and protons but a different number of neutrons. C1

5. The periodic table contains all the known elements.
The columns are numbered groups.
All the elements in a group have similar properties. 1 2 3 4 5 6 7
The group number of an element tells you how many electrons are in its outer shell.

6. Early Periodic Table What did John Newlands do?
Arranged in order of atomic mass.
Nowadays we know about protons so we arrange in order of ____________.
The outer shell electrons determine the ______number and the chemical properties.
Law of octaves: every 8th was similar
atomic number
Didn’t leave gaps for new elements!
What did Dmitri Mendeleev do?
group
Put them in order of atomic mass.
Arranged into groups with similar properties. C1
Left gaps for new elements and correctly predicted their properties!

7. Why are alkali metals so reactive?
Let’s look at Potassium:
Inner shell electrons shield the positive pull
Reaction with water
Metal + Water …………………...+…………………
Electronic configuration: __________
2,8,8,1
Metal hydroxide
hydrogen
A lone electron? Odd one out.
This electron is far from the _________ pull of the nucleus and very _____ to remove.
positive C1
easy

8. F Cl Br I Liquid Solid The Halogens (group 7) Group 0 Gas
Moving down the group:
Melting point _________, boiling point ________and reactivity____________.
the noble gases are very………………..
Because they have a …………………………..
Group 0
increases
increases
decreases F
Very reactive
Gas
Liquid
Solid
Unreactive Cl
Full outer shell of electrons Br I C1
A little reactive

9. Transition metals often form colourful compounds:
The ions can have different charges
Lower reactivities
Manganese ores
High melting points
High densities
Copper ores
Zinc ores
Good catalysts
Very typical metals
Alkali metal salts are boring and white.
Titanium ores

10. positive negative ionic zero high solution
Atoms and Ions
Ions are formed when atoms gain or lose electrons.
Magnesium has two electrons on its outer shell.
When it forms an ion, it loses these electrons to gain a full outer shell.
Metals always form ____________ ions and non-metals form _______________ ions.
Oppositely charged ions attract and form ___________ bonds.
The overall charge in an ionic compound is always ________
Ionic compounds have ______ boiling points and melting points.
Ionic compounds conduct electricity if they are………… or in …………………
positive
negative
ionic
Chlorine has seven electrons on its outer shell.
When it forms an ion, it gains an extra electron to fill its outer shell.
zero
high
Molten
solution C2

11. Giant Covalent Compounds
Graphite
Made of _________
Each carbon atom forms ________ bonds
Has ___________ electrons
Has weak intermolecular forces between layers which makes it ______.
Diamond
Made of carbon
Each carbon atom forms _______ bonds
Has no delocalised electrons
Has ______________ between all the carbon atoms which makes it hard.
Covalent Bonds
Form between non-metals when they share electrons to fill their outer shells.
carbon
three
delocalised
soft
Simple covalent compounds have very low melting and boiling points because there are weak intermolecular forces between them.
four
Strong bonds C2

12. Metals and their Properties+ + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + +
Metallic bonds are positive metal i___ surrounded by a sea of free-moving (d________) negative e______.
Metals can conduct electrical current because the charge (e-) can f__.
They conduct heat, can be bent into shape (m______) because layers can s___ over each other.
ons
elocalised
lectrons
low
alleable
lide C2

13. Pure metals aren’t as strong as alloys:
Easy for metal layers to slide over each other:
STRESS
Mix of different size particles in alloys make it harder for chains to slide over each other:
= Alloy mixture
STRESS C2

14. Exothermic reactions: Endothermic reactions:
Energy taken in
The products have more energy than the reactants.
Energy given out
Reactants have more energy than the products
Making bonds is ………………
Breaking bonds is ………………
exothermic
endothermic

15. Starting a reaction: Energy / kJ Progress of reaction
Activation energy
Smaller activation energy when catalyst is used
Energy / kJ
Reactants A + B
Progress of reaction
Products C + D

16. More Reactions Reactions and Rates C6
Reactions that take in heat are ____________
Reactions that give out heat are ___________
This symbol means that a reaction is _________
For a reaction to happen, molecules need to collide with enough energy, called activation energy.
If we give the reactants more energy, by heating, they will move faster and collide more frequently.
If we increase the concentration of the reactants, there will be more frequent collisions.
If we increase the surface area, of the reactants, there will be more frequent collisions.
If we increase the pressure of reacting gases, there will be more frequent collisions.
Endothermic
Exothermic
Reversible

17. Catalysts Catalysts s____ up the rate of chemical reactions.
They do no get c_____ by the reaction and can be re-used.
Catalysts lower the a_______ e____ of a reaction.
peed
hanged
ctivation
nergy