Module 2 Flashcards
1
Q
What does the mass number of an atom tell you about the sub-atomic particles?
A
Number of neutrons and protons.
2
Q
What does the atomic number tell you about the sub-atomic particles?
A
Number of protons.
3
Q
What is located in the centre of an atom?
A
Protons and neutrons.
4
Q
What is the centre of an atom called?
A
Nucleus
5
Q
What is the relative charge and mass of a proton?
A
Charge: +1
Mass: 1
6
Q
What is the relative charge and mass of a neutron?
A
Charge: 0
Mass: 1
7
Q
What is the relative charge and mass of an electron?
A
Charge: -1
Mass: 1/2000
8
Q
Which sub-atomic particle changes when ions are formed?
A
Electrons
9
Q
What type of ion will form when electrons are lost?
A
Positive ion
10
Q
What type of ion will form if electrons are gained?
A
Negative ion
11
Q
What is the definition of relative isotopic mass?
A
The mass of an atom of an isotope compared with 1/12th the mass of an atom of carbon-12.
12
Q
What is the definition of relative atomic mass?
A
The weighted mean mass of an atom of an element compared with 1/12th the mass of an atom of a carbon-12.
13
Q
What is the formula and charge of the carbonate ion?
A
CO3, 2-
14
Q
What is the formula and charge of the sulphate ion?
A
SO4, 2-
15
Q
What is the formula and charge on the hydroxide ion?
A
OH, -
16
Q
What is the formula and charge on the ammonium ion?
A
NH4, 1+
17
Q
What is the formula and charge on the nitrate ion?
A
NO3, 1-
18
Q
What is the charge on a zinc ion?
A
2+
19
Q
What is the charge on a silver ion?
A
1+
20
Q
What does the group number from the Periodic Table tell you about an atom?
A
Number of outer electrons.
21
Q
What are the units for amount of substance?
A
Mole (mol)
22
Q
What is the equation for calculating the number of atoms/particles/molecules?
A
Number of particles = moles x Avogadro’s number
23
Q
What is the equation for calculating mass?
A
Mass = Mr x mole
24
Q
What is the equation for calculating concentration?
A
Concentration = moles/volume
25
What is the equation for calculating volume of a gas?
Volume = moles x 24 (in dm3)
26
What is the definition of an anhydrous salt?
A salt that contains no water molecules.
27
What is the definition of a hydrated salt?
A crystalline salt containing water molecules.
28
What is the definition for water of crystallisation?
Water molecules that form an essential part of the crystalline structure of a compound.
29
What is the ideal gas equation?
pV = nRT
30
When can atom economy be 100%?
When only one product is formed.
31
What are some of the reasons why percentage yield may not be 100%?
1. Reaction may not go to completion.
2. By-products may form.
3. Impurities
4. Some product/reactants can be left in apparatus.
5. Purifying products can lead to loss.
32
How can atom economy for a reaction be increased?
Finding a use for by-products.
33
What is the formula of hydrochloride acid?
HCl
34
What is the formula of nitric acid?
HNO3
35
What is the formula of sulphuric acid?
H2SO4
36
What is the formula of ethanoic acid?
CH3COOH
37
What is the definition of an isotope?
Atoms of the same element with different numbers of neutrons (different mass number).
38
What is meant by the term strong acid?
A proton donor which fully dissociates.
39
What is meant by the term weak acid?
A proton donor which only partially dissociates.
40
What types of compounds are considered to be bases?
Metal hydroxides, metal oxides, ammonia
41
What is the formula of ammonia?
NH3
42
What is the reaction equation for neutralisation?
H+ + OH- --> H2O
43
What is the generic equation for forming a salt from a carbonate?
Acid + carbonate --> salt + water + carbon dioxide
44
What is the generic equation for forming a salt from a base/alkali?
Acid + base --> salt + water
45
What is the generic equation for forming a salt from a metal?
Acid + metal --> salt + hydrogen
46
What is the oxidation number for an uncombined element?
Zero
47
What is the oxidation number for combined oxygen (not in a peroxide or with F)?
-2
48
What is the oxidation number for oxygen in a peroxide?
-1
49
What is the oxidation number of oxygen when combined with F?
+2
50
What is the oxidation number for combined hydrogen?
+1
51
What is the oxidation number for hydrogen in metal hydrides?
-1
52
What is the oxidation number of simple ions?
Charge on the ion
53
What is the oxidation number of combined fluorine?
-1
54
What needs to happen to the oxidation numbers for a neutral compound?
Add up to zero
55
What do the Roman numerals in compound names indicate?
Charge on element of oxidation number of element
56
What does the term oxidation mean?
The loss of electrons, loss of hydrogen, gain of oxygen or an increase in oxidation number.
57
What does the term reduction mean?
The gain of electrons, gain of hydrogen, loss of oxygen or a decrease in oxidation number.
58
How many electrons does the first shell hold?
2
59
How many electrons does the second shell hold?
8
60
How many electrons does the third shell hold?
18
61
How many electrons does the fourth shell hold?
32
62
What is the definition of an atomic orbital?
A region of space where it is likely that you will find two electrons, with opposite spins.
63
What is the shape of the s-orbital?
Spherical
64
What is the shape of the p-orbital?
Dumbbell
65
How many orbitals are there in an s-sub-shell?
1
66
How many orbitals are there in a p-sub-shell?
3
67
How many orbitals are there in a d-sub-shell?
5
68
What is special about the 4s orbital?
It fills and empties first (before the 3d).
69
What is the definition of ionic bonding?
The electrostatic attraction between oppositely charged ions.
70
How are ionic bonds formed?
Ions form from the loss and gain of electrons.
71
What type of structure are ionic compounds?
Giant lattice
72
Why do ionic compounds have high melting and boiling points?
Only strong electrostatic forces of attraction within the giant structure.
73
Why do ionic compounds conduct when molten or in solution?
Ions are mobile
74
Why are ionic compounds soluble in polar solvents?
The polar solvents attract the oppositely charged ions and pull the lattice apart. The larger the charges on the ions in the lattice the less soluble the compound.
75
What is the definition of covalent bonding?
Electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms.
76
What type of structure can covalent compounds have?
Simple or giant
77
Which elements take part in giant covalent compounds?
Carbon and silicon
78
Why do diamond and graphite have high melting and boiling points?
Only strong covalent bonds between atoms within the giant structure - diamond. Graphite has mostly strong bonds but with some weak intermolecular forces between layers.
79
Why do simple covalent structures have low melting and boiling points?
Weak intermolecular forces between molecules which are being overcome.
80
Why do most covalent compounds not conduct?
No mobile ions or delocalised electrons
81
What is meant by the term dative covalent bond?
A covalent bond formed where both electrons in the shared pair are donated by one atom.
82
What is the shape and bond angle in a molecule with 1 pair of bonded electrons and no lone pairs?
Linear, 180 degrees
83
What is the shape and bond angle in a molecule with 2 pairs of bonded electrons and no lone pairs?
Linear, 180 degrees
84
What is the shape and bond angle in a molecule with 3 pairs of bonded electrons and no lone pairs?
Trigonal planar, 120 degrees
85
What is the shape and bond angle in a molecule with 2 pairs of bonded electrons and 2 lone pairs?
Non-linear (bent, v-shaped), 104.5 degrees
86
What is the shape and bond angle in a molecule with 3 pairs of bonded electrons and 1 lone pair?
Pyramidal, 107 degrees
87
What is the shape and bond angle in a molecule with 4 pairs of bonded electrons and no lone pairs?
Tetrahedral, 109.5 degrees
88
What is the shape and bond angle in a molecule with 5 pairs of bonded electrons and no lone pairs?
Trigonal bipyramidal, 120 and 90 degrees
89
What is the shape and bond angle in a molecule with 6 pairs of bonded electrons and no lone pairs?
Octahedral, 90 degrees
90
What type of electrons repel the most?
Lone pairs (repel more than bonded pairs)
91
What is the definition of electronegativity?
A measure of the attraction of an electron in a covalent bond.
92
What does the Pauling value tell you about an element?
The strength of its electronegativity. Greater the value, the more electronegative.
93
What does it mean for a bond to be polar?
A covalent bond that has a permanent dipole due to a difference in electronegativity between bonded atoms.
94
What is needed for a molecule to be polar?
Polar bonds which do not cancel out due to symmetry.
95
What leads to intermolecular forces?
Constant random movement of electrons.
96
How are London (dispersion) forces formed?
1. Movement of electrons leads to unbalanced distribution.
2. Instantaneous dipole forms in the non-polar molecule.
3. This induces a dipole in a neighbouring molecule.
4. Weak attraction between the molecules.
97
What are the 3 examples of Van dear Waals' forces?
1. Permanent dipole - induced dipole
2. Permanent dipole - permanent dipole
3. London forces
98
What is meant by the term hydrogen bonding?
Permanent dipole - permanent dipole attraction between the hydrogen on a OH, NH or FH on one molecule and a lone pair on NOF of a different molecule.
99
How does hydrogen bonding explain why ice is less dense than water?
Forms an open lattice with hydrogen bonds holding the water molecules apart.
100
How does hydrogen bonding explain why water has a higher melting and boiling point than expected?
Hydrogen bonds are stronger than other intermolecular forces meaning more energy is needed to overcome them.
