Topic 1 - Key Concepts

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Total cards: 24•Content version: v4•Public deck•Updated: 8/1/2026

Card preview (24)

Front (Question)

Ammonia formula

Back (Answer)

NH3

Front (Question)

Ammonium ions formula

Back (Answer)

NH4+

Front (Question)

Nitrate formula

Back (Answer)

NO3-

Front (Question)

Sulfate formula

Back (Answer)

SO4 2-

Front (Question)

Hydroxide formula

Back (Answer)

OH-

Front (Question)

Carbonate formula

Back (Answer)

CO3 2-

Front (Question)

Ionic equation

Back (Answer)

If a substance is ionic and aq, then it can be split into its individual ions to get he equation.

Front (Question)

Atom models

Back (Answer)

Dalton model - solid spheres, JJ Thompson - Electrons inside sphere(plum pudding model), Rutherford - Positive nucleus, electrons float, Bohr - electron shells

Front (Question)

Nucleus size and mass

Back (Answer)

Tiny compared to rest of atom but most of the mass in the atom is inside it

#10

Front (Question)

Mass number

Back (Answer)

Total number of protons and neutrons in an atom

#11

Front (Question)

Atomic number

Back (Answer)

Proton amount. Amount of protons is unique to each atom.

#12

Front (Question)

Isotope

Back (Answer)

An atom with the same number of protons but a differetn number of neutrons in the nucleus. There are different isotopes for some different elements, which leads to their mass numbers not being whole.

#13

Front (Question)

Relative atomic mass calculation based on isotopic abundances

Back (Answer)

Multiply each isotope mass by its quantity. Then add all of them upp and divide by the sum of the quantities.

#14

Front (Question)

How did mendeleev arrange his table

Back (Answer)

Based on atomic mass which put elements with similar properties in columns. Some were wrong due to isotopes, and gaps were left for undiscovered elements, which he predicted the properties of.

#15

Front (Question)

Periodic table arrangement now

Back (Answer)

Ascending atomic number, rows called periods which represent shells on the atom, columns called groups which have elements with similar properties

#16

Front (Question)

Ionic bonding

Back (Answer)

When a metal and non-metal bond by the metal losing electrons and giving them to the non-metal. The oppositely charged ions are strongly attracted to eachother by electrostatic forces.

#17

Front (Question)

Ionic compounds properties

Back (Answer)

Lattice structure, high melting and boiling points, delocalised electrons so can carry electric charge

#18

Front (Question)

Covalent bonding

Back (Answer)

When a pair of electrons is shared between two atoms. Leads to formation of molecules( around 10 power -10 m size)

#19

Front (Question)

Giant covalent structures

Back (Answer)

Large molecules held by strong covalent bonds. High boiling and melting points. Dont conduct electricity. Eg diamonds, graphite, graphene(all forms of carbon)

#20

Front (Question)

Metallic bonding

Back (Answer)

Giant structures held very strongly together by electrostatic attraction between positive metal ions and electrons.

#21

Front (Question)

Graphite

Back (Answer)

Three covalent bonds creating sheets of carbon atoms arranged in hexagons. The sheets slide over eachother meaning it is soft and slippery. Used for lubricants

#22

Front (Question)

Diamond

Back (Answer)

Network of carbon atoms that from 4 covalent bonds. Rigid lattci structure leads to it being really hard. Used to strengthen cutting tools

#23

Front (Question)

Fullerenes

Back (Answer)

Molecules of carbon in closed tubes or hollow balls.

#24

Front (Question)

Buckminsterfullerene

Back (Answer)

C60. Forms a hollow sphere made of 20 hexagons and 12 pentagons. Stable molecule that forms soft crystals.