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Chemistry > Unit 2 - Mrs Richards > Flashcards

Unit 2 - Mrs Richards Flashcards

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1
Q

Define Molecular mass (Mr)

A

Mass of the atoms in a given formula

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2
Q

Define Avagardo’s Constant

A

It is 6.02 x 10^23. In one mole of ANYTHING, there is always 6.02 x 10^23 of something in it, be it electrons, atoms or molecules.

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3
Q

What is one mole of an element the same as?

A

the Ar in gmol-1

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4
Q

Define empirical formula

A

The simplest whole number ratio of atoms of each element present in a compound

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5
Q

Define Molecular formula

A

The actual number of atoms of each element in a compound

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6
Q

What is the formula of ethanoic acid?

A

CH3COOH

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7
Q

Define atom economy

A

A measure of how much of the products are useful

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8
Q

What type of reaction do we have if the atom economy is 100%

A

An addition reaction

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9
Q

What type of reaction do we have if the atom economy a bit less than 100%

A

A substitution reaction

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10
Q

What type of reaction do we have if the atom economy is a lot less than 100%

A

An elimination reaction

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11
Q

Define an acid

A

They are chemical agents that release hydrogen ions when it is added to water, hydrogen DONATORS

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12
Q

What is the difference between strong and weak acids?

A

Depends on how IONISED it is in water. A strong acid 100% ionised and has a pH of 1, a weak acid is only partly ionised and has a pH of 3-5

SAME FOR ALKALIS (strength depends on how ionised it is)

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13
Q

Define a base

A

A base is a substance that will neutralise an acid, but does not dissolve in water. t is a H+ ion acceptor

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14
Q

Define an alkali

A

It is any substance that produces hydroxide OH- ions when added to water.

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15
Q

Write the ionic equation for the reaction of an acid with any alkali

A

H+ + OH- —> H2O

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16
Q

Name a strong alkali

A

sodium hydroxide solution or calcium hydroxide solution (limewater)

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17
Q

Name a weak alkali

A

Ammomnia

18
Q

How do you complete a titration?

A

See textbook

19
Q

What would the oxidation state of N be?

A

0, as are all elements

20
Q

What would the oxidation state of Fe3+ be?

A

+3

21
Q

What would the oxidation state of H be in a compound?

A

+1
Only exceptions are - 0 as H or H2
- -1 as a hydride ion, H- and in sodium hydride
NAH

22
Q

What would the oxidation state of O be in a compound?

A

-2
Only exceptions are - 0 as O or O2
- -1 in Hydrogen Peroxide, H2O2
- +2 in F2O

23
Q

What would the oxidation state of F be in a compound?

A

-1

The exception is - as F or F2

24
Q

What must all the oxidation numbers in the compound total?

A

The overall charge of the compound

25
Q

Define Redox

A

When reduction and oxidation take place

26
Q

If the oxidation state increases, has the element been oxidised or reduced?

A

Oxidised

27
Q

If the number of electrons has decreased, has the compound being oxidised or reduced?

A

oxidised, so it will become more positive

OILRIG

28
Q

What do we use to balance redox reactions?

A

electrons, H and H2O

29
Q

How do you combine half equations?

A

1) Write the out
2) Multiply the equations so that the number of electrons in each is the same
3) Add the 2 equations and cancel out the electrons on either side
4) If necessary, cancel any other species which appear on both sides

30
Q

Define Relative Atomic Mass

A

The weighted mean mass of an atom of an element compared with 1/12 the mass of carbon -12

31
Q

Define a mole

A

The amount of any substance that contains the same number of particles as there are carbon atoms in 12g of carbon -12

32
Q

What is the formula for the number of particles present in an atom?

A

n x (6.02 x 10^23)

33
Q

What is the difference between an atom and a molecule

A

A molecule is made up of atoms

34
Q

What do we do with percentages when working out empirical formulas?

A

Treat them as just grams

35
Q

What is 24dm^3 often referred to as?

A

The molar gas volume

36
Q

What do chemists call strong solutions?

A

Concentrated

37
Q

What do chemists call weak solutions?

A

Dilute

38
Q

Define concentration

A

The number of moles dissolved per dm^3 of solution

39
Q

Why are standard solutions used for titration?

A

We know the concentration and can use this to work out the moles, hence been able to work out the concentration of the alkali

40
Q

What unit must all values be when dividing by the Mr?

A

Grams

41
Q

How many grams is 1 tonne

A

1000000 or 1x10^6

Chemistry (9 decks)

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