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Chemistry > Foundations In Chemistry > Flashcards

Foundations In Chemistry Flashcards

(I) Atomic structure (II) Quantitative chemistry: formulae, equations, amount of substance and the mole (III) Reactions of acids (IV) Oxidation number and redox reactions (V) Bonding and structure.

1
Q

What are the sub particles of an atom?

A

Protons, Electrons, Neutrons

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2
Q

What are the charges on the sub particles?

A

Protons- Positive (+)
Electrons- Negative (-)
Neutrons- Neutral

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3
Q

Where are they found in an atom?

A

Protons - In the nucleus
Electrons - On shells that are orbiting the nucleus
Neutrons- In the nucleus

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4
Q

What is the overall charge of the nucleus?

A

Positive because it has protons

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5
Q

What is the overall charge of an atom?

A

An atom is neutral because it has the same number of protons and neutrons

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6
Q

What is the Atomic number(Z) of an element?

A

It is the number of protons in an atom

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7
Q

What is the Mass number (A) of an element?

A

It is the proton number (Z) + the neutron number (N) in the nucleus of an atom

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8
Q

What are isotopes?

A

Isotopes are atoms with the same number of protons but different number of neutrons and different mass numbers

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9
Q

What is the relative isotopic mass of an element?

A

It is the mass of an atom of an isotope compared with 1/12th of an atom of carbon

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10
Q

What is the relative atomic mass of an element?

A

It is the weighted mean mass compared with 1/12th mass of carbon-12

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11
Q

Equation to calculate Ar

A

sum of (isotopic abundance * isotopic mass number) ➗ 100

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12
Q

Formula and charges on some complex ions
LEARN THESE

A

Nitrate - NO3
Sulphate - SO3
Carbonate - CO3
Ammonium - NH4
Hydroxide - OH-

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13
Q

What is a mole?

A

A mole contains 6.02 x10^23 atoms, ions or molecules as there are in exactly 12g of carbon-12

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14
Q

What is Molar Mass?

A

It is the Mass of one mole of a substance. Its units are g/mol^-1

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15
Q

Formula for calculating moles

A

Moles= mass/Mr

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16
Q

Formula for measuring concentration

A

Concentration=moles/volume

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17
Q

Units for concentration

A

mol/dm^3

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18
Q

What is the Molar gas volume?

A

One mole of any gas at room temperature and pressure has a volume of 24dm^3

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19
Q

Equation for calculating moles with Molar gas volume

A

Moles=volume given/Molar gas volume (dm^3)

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20
Q

What does a volume of a gas depend on?

A

The pressure applied to the gas
The temperature of the gas
Number of moles of a gas

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21
Q

What is the ideal gas equation?

A

pV=nRT where;
p=Pressure (Pa)
V= Volume (m^3)
n= number of moles
R=ideal gas constant
T= temperature(K)

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22
Q

What is an acid?

A

A species that can donate protons (H+ ions)

23
Q

What is a base?

A

A species that can accept protons (via lone pair)

24
Q

What is an alkali?

A

It is a base that is soluble in water

25
Q

What are strong acids/bases?

A

They fully dissociate to release H+ ions in aqueous solutions

26
Q

What are weak acids/base?

A

They do not fully dissociate to release their ions in aqueous solutions

27
Q

Examples of common acids

A

HCl- Hydrochloric acid
H2SO4- Sulphuric acid
HNO3- Nitric acid
CH3COOH- Ethanoic acid

28
Q

Examples of common alkalis

A

Sodium hydroxide- NaOH
Potassium hydroxide- KOH
Ammonia- NH3

29
Q

Reaction of acid with alkali

A

Acid + Alkali - Salt + Water

30
Q

Reaction of acid with metal oxide

A

Acid + Metal oxide - salt + water

31
Q

Reaction of acid with metal hydroxide

A

Acid + metal hydroxide - salt + water

32
Q

Reaction of acid with metal carbonate

A

Acid + metal carbonate- salt + water + Carbon dioxide

33
Q

Reaction of acid with metals

A

Acid + metals - Salt + hydrogen

34
Q

What is an atomic orbital?

A

It is a region around the nucleus that can hold up to 2 electrons with opposite spins

35
Q

What are the 4 subshells?

A

S,P,D and F

36
Q

What is the shape of the s subshell?

A

Spherical

37
Q

What is the shape of the p subshell?

A

dumbbell shaped

38
Q

How many orbital does the s subshell have?

A

1

39
Q

How many orbitals does the p subshell have?

A

3

39
Q

How many orbital does the d subshell have?

A

5

40
Q

How many orbital does the f subshell have?

A

7

41
Q

What is an ionic bond?

A

It is the electrostatic force of attraction between oppositely charged ions

42
Q

What type of element does ionic bonding occur between?

A

It occurs between metals and nonmetals

43
Q

What type of structure do the ions form in ionic bonding?

A

The ions form a giant ionic lattic

44
Q

What are some properties of ionic compounds?

A

1.They have high MP and BP
2.They only conduct electricity when molten or dissolved
3.They can dissolve in water

45
Q

Why do ionic compounds have high MP and BP?

A

This property is due to the strong electrostatic force of attraction between the oppositely charged ions which require a lot of energy to break

46
Q

Why do ionic compounds only conduct electricity when molten or dissolved?

A

This is because when the ionic compounds are in their solid state, the ions are not free to move as they are in fixed positions in the lattice but when molten, the ions are free to move and can carry charge

47
Q

Why do ionic compounds dissolve in water?

A

Water is a polar solvent(1)and the ions in the lattice are attracted to the dipole charges: Na+ to O- and Cl- to H+ (1)breaking the ionic bonds(1)

48
Q

What is a covalent bond?

A

It is a shared pair of electrons

49
Q

What is covalent bonding?

A

It is the electrostatic force of attraction between the shared pair of electrons and the nuclei of the bonded atoms

50
Q

What type of elements does covalent bonding happen between?

A

Covalent bonding happens between non-metals and non-metals

51
Q

What is a dative covalent bond?

A

It is a shared pair of electrons in which both of the electrons come from the same atom

52
Q

What are lone pairs of electrons?

A

They are paired electrons that are not involved in bonding

Chemistry (3 decks)

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