Chemistry A-level (module 2)

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45 Terms

1
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What was the order the atom models were produced in?

  1. Atomic model

  2. Plum pudding model

  3. Nuclear model

  4. Bohr model

2
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Who was responsible for the atomic model (and what was newly discovered)?

John Dalton (atoms)

3
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Who was responsible for the plum pudding model (and what was newly discovered)?

JJ Thompson (electrons)

4
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Who was responsible for the nuclear model(and what was newly discovered)?

Rutherford (nucleus)

5
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Who was responsible for the Bohr model (and what was newly discovered)?

Niels Bohr (shells)

6
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What is the relative charge (RC) & relative mass (RM) of protons, neutrons and electrons?

Proton:

  • RC = 1+

  • RM = 1

Neutron:

  • RC = 0

  • RM = 1

Electron:

  • RC = 1-

  • RM = 1/1836

7
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What is relative atomic mass?

The average mass of an atom relative to 1/12th of a carbon atom

8
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What is a binary compound?

  • 2 elements only

  • Metal element comes first

  • The ending of the 2nd element changes to -ide

9
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What is a polyatomic ion?

More than one elements make up an ion

10
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What are the first 6 prefixes to use when naming a molecular compound?

1 - mono

2 - di

3 - tri

4 - tetra

5 - Penta

6 - hexa

11
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What is the molecular formula?

The number and type of atoms of each element covalent bonded together in a molecule

12
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What is the empirical formula?

Simplest whole number ration of atoms of each element present in a compound

  • always used for ionic compounds

  • Some molecular formula can be simplified

13
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How many electrons are in each of the first 4 shells?

1) 2

2) 8

3) 18

4) 32

14
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What is the formula to work out the maximum number of electrons in a shell?

2n²

15
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What is an atomic orbital?

A region around the nucleus that can hold up to 2 electrons with opposite spins

16
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What are the different types of orbitals and is one key difference?

S-, p-, d-, f- orbitals

  • their shapes are different

17
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What is the principle quantum number (n)?

The shell number of energy number

18
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What is an electron cloud?

How electrons are found, represented by orbitals

19
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What is the shape of an s-orbital?

Sphere

20
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how many electrons can an s-orbital contain?

2 in each orbital

  • starts at n=1

21
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Why can transition metals form multiple ions?

They can lose different amounts of electrons due to their orbitals

22
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What is the shape of a p-orbital?

Dumb bell

23
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How many electrons can a p-orbital contain?

6 in each orbital

  • starts at n=2

24
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How many electrons can a d- orbital contain?

10 in each orbital

  • starts at n=3

25
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How many electrons can an f-orbital contain?

14 in each orbital

  • starts at n=4

26
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What is the electronic configuration of Helium (He)?

1S² (2)

27
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What is the electronic configuration of Neon (Ne)?

1S² 2S² 2P^6 (10)

28
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What is the electronic configuration of argon (Ar)?

1S² 2S² 2P^6 3S² 3P^6 (18)

29
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What 3 elements can be used in the shorthand versions of electronic configurations?

Helium [He], Neon [Ne], Argon [Ar]

30
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What are the 2 conditions for ionic compounds to dissolve in water?

  • attraction to solvent must be stronger than the bonds

  • Solvent molecules surround ions

31
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What do ideal gasses assume?

  • intermolecular forces of attraction are negligible

  • Size of gas molecules is negligible compared to size of container

  • Random motion and elastic collisions of molecules (no kinetic energy is lost during collisions)

32
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What is Avogadro’s law and what is a good analogy to remember it?

V is proportional to n

  • If you want to add more words, you’ll need a bigger book

33
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What is Charle’s law and what is a good analogy to remember it?

V is proportional to T

  • if you increase the spacing between words you’ll need a bigger book

34
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What is Boyle’s law and what is a good analogy to remember it?

P is not proportional to V

P is proportional to 1/V

  • if an elephant steps on the book, the book will get smaller and words will get closer together

35
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What is Gay-Lussac’s law (aka Amonton’s law) and what is a good analogy to remember it?

P is proportional to T

  • if you give the words more energy they’ll try to jump off the page more, putting more pressure on the binding

36
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What is the ideal gas equation (+ units for each)?

PV = nRT

P = pressure (Pa)

V = volume (m³)

n = moles

R = gas constant (8.31 J K^-1 mol^-1)

T = temperature (K)

37
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What is meant by absolute 0 degrees?

0 Kelvin (-273 ° C)

  • all particles stop vibrating

  • Complete absence of heat energy

38
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What is the definition of concentration?

How much solute is in a known volume of a solution

39
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What is the equation of concentration?

Concentration = moles/ volume

= mass/ volume

40
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What is a standard solution?

A solution of known concentration

41
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What are the standard conditions and what is the volume of 1 mole at these conditions?

RTP - room temperature and pressure

  • temp = 20° C

  • Pressure = 101 kPa ( 1 atm)

  • 1 mole has a volume of 24 dm³

42
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What is the formula for using moles and RTP?

V = moles x RTP

V = dm³

RTP = 24

43
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What kind of pairs of electrons have the greatest repulsion?

Lone pair to lone pair repulsion

44
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What kind of pair of electrons have the weakest repulsion?

Bond pair to bond pair repulsion

45
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What kind of pairs of electrons has the middle repulsion?

Lone pair to bond pair repulsion