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Chemistry > Module 2 > Flashcards

Module 2 Flashcards

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1
Q

What is ionisation

A

Turning an atom/element Into an ion specifically positive ion

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2
Q

Give an equation to represent ionisation

A

X (g) -> X* (g). + e-

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3
Q

What are the two axis of a mass spectrum

A

-relative abundance
-m/z (mass charge ratio)

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4
Q

What is the isotopic mass of an atom

A

Mass of an isotope relative to 1/12th of an atom of C-12

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5
Q

What is the relative atomic mass

A

Weighted mean mass of an element when compared to C-12 when C-12 has a mass of 12

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6
Q

Relative atomic mass equations

A

(Mass number x %) + ( mass number x %)
———————————————————-
100

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7
Q

What is an orbital

A

Region of space that electrons are most likely to be in around the nucleus

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8
Q

What are the 4 types of orbitals in order

A

S, P, D and F

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9
Q

How many electrons can occupy any one orbital and what spin will they have

A

2 electrons and they’ll have opposite spin

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10
Q

What do orbitals make

A

Sub shells

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11
Q

What shape is an s orbital

A

Sphere

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12
Q

What shape is a P orbital

A

Dumbbell

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13
Q

How many p orbitals make a p subshell

A

3p

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14
Q

How many d orbitals make a d subshell

A

5

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15
Q

How many s orbitals make a s subshell

A

1

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16
Q

How many f orbitals make an f subshell

A

7f

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17
Q

What is quantum level 1 made up of

A

S subshell with 2 electrons

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18
Q

What is quantum level 2 made up of

A

2 sub shells (2s 2p)
One s orbital in the subshell with 2 electrons
Three p orbitals in the p subshell with 6 electrons

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19
Q

What is the electrons configuration for sodium (Na)

A

2,8,1:
1S^2 2S^2 2P^6 3S^1

20
Q

rules for filling the orbitals

A
  1. Electrons enter the lowest energy orbital available
  2. -electrons fill the next singly occupied orbital
    -electrons only share orbitals when there are no empty orbitals in the subshell
21
Q

What is the relative molecular mass

A

Sum of relative atomic mass of all the atoms in a molecule of a compound (Mr)

22
Q

What is a mole

A

Unit for amount of a substance containing as many particles as there are carbon atoms in exactly 12g of the C-12 isotope

23
Q

What is avogadros constant

A

6.02 x 10^23

24
Q

How many molecules of copper sulphate are in 1 mol of copper sulphate

A

6.02 x 10^23

25
Q

Reacting mass calculation when given 1 mass order or working

A
  1. Mol of known (mass/mr)
  2. Mol ratio (mol : unknown)
  3. Mass of unknown (mol x Mr)
26
Q

Limiting reagent calculation when given two masses order of calculation

A
  1. Mol of both given reagents (mass/mr)
  2. Mol ratio to find limiting reagent
  3. Mol known from step 1
  4. Mol ratio (limiting : unknown)
  5. Mass unknown (mol x Mr)
27
Q

What is the empirical formula

A

Simplest whole number ratio of each element present ina compound

28
Q

What is the molecular formula

A

Actual number of atoms of each element in a compound

29
Q

Method for working out the empirical formula when given mass or percentages

A

In a table
1. Write mass or percentage of each element
2. Mind mol (mass/Ar) for each element
3. Find ratio (divide both by smallest mol)
4. Whole number ratio
5. Formula

30
Q

What is the standard notation for displaying the electronic structure when drawing the electrons in orbitals

A

An arrow up and an arrow down each showing an electrons and the opposite spins

31
Q

Which two elements have different electron configurations

A

Copper and chromium
Cu and Cr

32
Q

Why do Cr and Cu have different electron configurations

A

More stable with a half full or full subshell of 3drather than in 4S

33
Q

Electron configuration for Cr

A

1s^2 2s^2 2p^6 3s^2 3p^6 4s^1 3d^5

34
Q

Electron configuration for Cu

A

1s^2 2s^2 2p^6 3s^2 3p^6 4s^1 3d^10

35
Q

anhydrous meaning

A

Substance that contains no water molecules

36
Q

Hydrated meaning

A

Crystalline and containing water molecules

37
Q

Water of crystallisation meaning

A

Water molecules that form an essential part of the crystalline structure of a compound

38
Q

How to do a calculation of the formula of a hydrated salt ( water of crystallisation) when given percentage composition, mass composition or based on results

A
  1. Mol of anhydrous (mass/mr)
  2. Mol of water (mass/mr)
  3. Ratio using mol
39
Q

Limiting reagent?

A

Substance in a chemical reaction that runs out first

40
Q

What is room temperature pressure

A

208k and 101kPa

41
Q

Equation mol of gas

A

Number of moles = volume in dm^3/24

42
Q

What does a 1 mol dm^3 solution mean

A

Solution contains 1 mol of solute dissolved in each 1 dm^3 of solution

43
Q

Equation for moles for solution

A

Mol = conc x vol

44
Q

What is the ideal gas equation

A

pV=nRT

45
Q

What do the letter in the ideal gas equation stand for

A

p=pressure, V=volume, n=mol of gas, R=ideal gas constant, T=temperature

46
Q

Units in the ideal gas equation

A

p=Pa, V=m^3, n=no units, R= 8.314, T=K

Chemistry (6 decks)

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