chemistry 🧪

yr10 chemistry

Group vs Period

Group = vertical column
Period = horizontal row

Alkali Metals

Group 1, very reactive, soft, react with water
Example: Lithium, Sodium

Alkaline Earth Metals

Group 2, reactive (less than group 1), harder
Example: Magnesium, Calcium

Transition Metals

Middle of table, strong, high MP, conduct electricity
Example: Iron, Copper

Halogens

Group 7/17, very reactive non-metals, form salts
Example: Fluorine, Chlorine

Noble Gases

Group 18, unreactive, full outer shell
Example: Helium, Neon

Ionic bonding

Metal + non-metal, transfer electrons

Covalent bonding

Non-metal + non-metal, share electrons

Metallic bonding

Metal atoms + sea of electrons

naming Ionic compounds

Metal + non-metal (-ide)
Example: Sodium chloride

naming covalent compounds

Use prefixes (mono-, di-, tri-)
Example: Carbon dioxide

law of conservation of mass

Mass is not created or destroyed in a reaction

what type of ions does an ACID release

releases H+ ions

what type of ions does a BASE release

releases OH- ions

litmus paper?

Acid = red
Base = blue

what does a universal indicator do?

shows pH scale

Exothermic

Releases heat
Example: Combustion

Endothermic

Absorbs heat
Example: Photosynthesis

acid + metal reaction, how can we test it?

= salt + hydrogen
Hydrogen test →
“Pop” sound with flame

acid + base

Salt + Water (neutralisation)

Acid + Carbonate, how can we test it?

Salt + Water + CO₂

CO₂ test →
Limewater turns milky

Corrosion reaction

Metal + oxygen → oxide
Example: Rusting

combustion reaction

Fuel + oxygen → CO₂ + H₂O

precipitation

two solutions → solid forms

example reaction

Magnesium hydroxide + hydrochloric acid →
Magnesium chloride + water

Reaction type →
Neutralisation

how does surface area change reaction rate

More area = faster reaction

how does concentration change reaction rates

Higher = faster

temperature change reaction rates

Higher = faster

how does a catalyst change reaction rate

it speeds up the reaction

how does agitation change reaction rates

mixing = faster reaction

what is collision theory

Particles must collide with enough energy to react

what type of compound does METAL + NONMETAL cause

ionic

what type of reaction does NON-METAL + NON-METAL cause

covalent

more collisions = ?

faster reaction

full outer shell = ?

stable atom

Nucleus

Center of atom contains protons and neutrons

Electron shells

Energy levels where electrons are found

Element

Pure substance with one type of atom

Valency

Number of electrons in outer shell

Group from valency

Same valency means same group

Period from shells

Number of shells equals period

Electron configuration

Arrangement of electrons in shells

First 20 rule

2 8 8 2

Ion

Charged particle

How ions form

Gain or lose electrons

Cation

Positive ion lost electrons

Anion

Negative ion gained electrons

Group 1 charge

+1

Group 2 charge

+2

Group 6 charge

-2

Group 7 charge

-1

Group 1 reactivity

Increases down the group

Group 2 reactivity

Increases down the group

Metallic bonding structure

Positive ions in sea of delocalised electrons

Ionic bonding structure

Lattice of oppositely charged ions

Covalent bonding structure

Shared electron pairs between atoms

Ionic formula

Balance charges to make neutral

Covalent formula

Based on number of atoms using prefixes

Metal displacement

More reactive metal replaces less reactive

Complete combustion

Fuel plus oxygen makes carbon dioxide and water

Incomplete combustion

Fuel plus limited oxygen makes carbon monoxide carbon and water

Oxygen test

Glowing splint relights

Neutralisation real life

Antacids treat stomach acid

Bee or wasp stings

Opposite pH neutralises

Rate of reaction

How fast reactants turn into products

Measuring rate

Change in amount over time

Rate graph steep

Fast reaction

Rate graph flat

Reaction finished

Enzyme

Biological catalyst

Lock and key model

Substrate fits exactly

Induced fit model

Enzyme changes shape slightly

Higher temperature effect

More energy more successful collisions

Higher concentration effect

More particles more collisions

Surface area effect

More exposed particles more collisions

Catalyst effect

Lowers activation energy

Balanced equation

Same number of atoms on both sides

Charge balance

Ionic compounds must be neutral

Faster reaction meaning

More successful collisions per second