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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. (70 cards)

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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 electrons

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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 - SO4 2-
Carbonate - CO3 2-
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)

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23
Q

What is a base?

A

A species that can accept protons (via lone pair)

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24
Q

What is an alkali?

A

It is a base that is soluble in water

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25
What are strong acids/bases?
They fully dissociate to release H+ ions in aqueous solutions
26
What are weak acids/base?
They do not fully dissociate to release their ions in aqueous solutions
27
Examples of common acids
HCl- Hydrochloric acid H2SO4- Sulphuric acid HNO3- Nitric acid CH3COOH- Ethanoic acid
28
Examples of common alkalis
Sodium hydroxide- NaOH Potassium hydroxide- KOH Ammonia- NH3
29
Reaction of acid with alkali
Acid + Alkali - Salt + Water
30
Reaction of acid with metal oxide
Acid + Metal oxide - salt + water
31
Reaction of acid with metal hydroxide
Acid + metal hydroxide - salt + water
32
Reaction of acid with metal carbonate
Acid + metal carbonate- salt + water + Carbon dioxide
33
Reaction of acid with metals
Acid + metals - Salt + hydrogen
34
What is the standard solution?
It is a solution of known concentration
35
What piece of equipment is used for making standard solutions?
Volumetric flasks
36
How to prepare a standard solution.
1. The solid is first weighed accurately 2. The solid is then dissolved in a beaker using distilled water. Use a glass rod to stir the solution to help the solid dissolve 3. The solution is then transferred to a volumetric flask and the last traces of the solution are rinsed into the flask using distilled water. 4. The flask is carefully filled to the graduation line with distilled water using a pipette until the bottom of the meniscus lines exactly with the mark 5. Put the lid over the flask and invert it several times to mix the solution
37
What is an atomic orbital?
It is a region around the nucleus that can hold up to 2 electrons with opposite spins
38
What are the 4 subshells?
S,P,D and F
39
What is the shape of the s subshell?
Spherical
40
What is the shape of the p subshell?
dumbbell shaped
41
How many orbital does the s subshell have?
1
42
How many orbitals does the p subshell have?
3
43
How many orbital does the d subshell have?
5
44
How many orbital does the f subshell have?
7
45
What is an ionic bond?
It is the electrostatic force of attraction between oppositely charged ions
46
What are ions?
Ions are atoms or groups of atoms that have either gained or lost e- to become positively charged (a cation) or negatively charged(an anion)
47
What type of element does ionic bonding occur between?
It occurs between metals and nonmetals
48
What type of structure do the ions form in ionic bonding?
The ions form a giant ionic lattic
49
What are some properties of ionic compounds?
1.They have high MP and BP 2.They only conduct electricity when molten or dissolved 3.They can dissolve in water
50
Why do ionic compounds have high MP and BP?
This property is due to the strong electrostatic force of attraction between the oppositely charged ions which require a lot of energy to break
51
Why do ionic compounds only conduct electricity when molten or dissolved?
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
52
Why do ionic compounds dissolve in water?
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)
53
What determines the solubility of an ionic compound in water?
1. The relative strength of the attractions within the giant ionic lattice; 2. The attraction between the ions and the water molecules
54
Why does the strength of the attractions within the giant ionic lattice affect solubility?
This is because the larger the charges, the harder it is for the water molecules to attract the oppositely charged ions and break down the lattice. Therefore, **solubility increases as ionic charge increases**
55
What is a molecule?
Molecules are groups of atoms that are bonded together.
56
What is a covalent bond?
It is a shared pair of electrons
57
What is covalent bonding?
It is the electrostatic force of attraction between the shared pair of electrons and the nuclei of the bonded atoms
58
What type of elements does covalent bonding happen between?
Covalent bonding happens between non-metals and non-metals
59
What is a dative covalent bond?
It is a shared pair of electrons in which both of the electrons come from the same atom
60
What are lone pairs of electrons?
They are paired electrons that are not involved in bonding
61
What does the average bond enthalpy measure?
It measures the energy needed to break a covalent bond
62
How does the value of the average bond enthalpy change as bond strength increases?
As bond strength increases, more energy is needed to break it, and so the value of the average bond enthalpy increases.
63
What is the Electron-pair repulsion theory?
It is a theory used to explain and predict the shapes of molecules and polyatomic ions
64
What effect do lone pairs have on the shape of molecules
Lone pairs repel more than bonding pairs so the angles between lone pairs of electrons are greater than the bond angles between bonding pairs
65
By how much does a lone pair reduce the bond angle of a bonding pair?
The bond angle of a bonding pair is reduced by **2.5°** for each lone pair.
66
What is a hydrogen bond?
It is an attraction between a lone pair of electron on an electronegative atom in one molecule and a hydrogen atom in another molecule
67
Anomalous properties of water
1. Ice is less dense than water. This is because the water molecules are held together by hydrogen bonds in an open lattice structure decreasing the density 2. High MP and BP. This is because the hydrogen bonds are really strong so a large amount of energy is needed to break them. 3. High surface tension and viscosity.
68
What is electronegativity?
It is the ability of an atom to attract the bonded pair of electrons in a covalent bond
69
Factors affecting electronegativity
Nuclear charge Atomic radius Number of electron shielding
70
How does nuclear charge affect electronegativity?
As the nuclear charge ⬆, the electronegativity ⬆. This is because the increased positive charge increases the attraction between the electrons in the outer shell

Chemistry (3 decks)

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