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Chemistry Edexcel > Topic 1 - Key Concepts > Flashcards

Topic 1 - Key Concepts Flashcards

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1
Q

Ammonia formula

A

NH3

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2
Q

Ammonium ions formula

A

NH4+

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3
Q

Nitrate formula

A

NO3-

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4
Q

Sulfate formula

A

SO4 2-

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5
Q

Hydroxide formula

A

OH-

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6
Q

Carbonate formula

A

CO3 2-

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7
Q

Ionic equation

A

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

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8
Q

Atom models

A

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

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9
Q

Nucleus size and mass

A

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

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10
Q

Mass number

A

Total number of protons and neutrons in an atom

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11
Q

Atomic number

A

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

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12
Q

Isotope

A

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.

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13
Q

Relative atomic mass calculation based on isotopic abundances

A

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

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14
Q

How did mendeleev arrange his table

A

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.

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15
Q

Periodic table arrangement now

A

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

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16
Q

Ionic bonding

A

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
Q

Ionic compounds

A

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

18
Q

Covalent bonding

A

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

19
Q

Giant covalent structures

A

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

20
Q

Metallic bonding

A

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

21
Q

Graphite

A

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
Q

Diamond

A

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

23
Q

Fullerenes

A

Molecules of carbon in closed tubes or hollow balls.

24
Q

Buckminsterfullerene

A

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

25
Q

Metal properties

A

Mostly very high melting and boiling points. In pure metals, layers of atoms can slide over eachother, making metals malleable. Good conductors.

26
Q

relative formula mass Mr =

A

All the atoms relative atomic masses in the formula

27
Q

What is empirical formula

A

The simplest ratio of atoms

28
Q

Law of consrvation of mass

A

No atoms are created or destroyed . In a closed system, the mass will stay the same

29
Q

What leads to the mass increasing during a reaction

A

The reactant is a gas in the air, so it is used by the reaction and more atoms are present in the product.

30
Q

What leads to mass decreasing during a reaction

A

When the product is a gas, it is released to the air and therefore the product has less atoms than the original reactants.

31
Q

Concentration unit

A

g dm-3

32
Q

Concentration =

A

Mass of solute / Volume of solution

33
Q

Avogadros constant shows

A

The amount of atoms in a mole

34
Q

Avogadros constant =

A

6.02 x 10^23

35
Q

Moles =

A

Mass(g) / Mr

36
Q

Particles of a substance =

A

Moles x 6.02 x 10^23

37
Q

How is the magnesium oxide experiment carried out to find empirical formula

A

Weight magnesium.
Heat it in a crucible whilst letting oxygen in until it turns white
Weigh the magnesium oxide
Use the masses and Mr of magnesium and oxygen to find the empirical formula

38
Q

Reactions stop when

A

The limiting reactant is used up

39
Q

The amount of product fromed is directionally proportional to

A

The amount of limiting reactant

Chemistry Edexcel (9 decks)

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