Unit 1 Flashcards
1
Q
What is the atomic number?
A
The number of protons in an atom’s structure.
2
Q
What is the mass number?
A
The number of protons + neutrons in the atom’s nucleus.
3
Q
Define Element.
A
Contains only one type of atom.
4
Q
Define isotope.
A
Atoms with the same atomic number but different mass number.
(same number of protons as electrons, but different number of neutrons)
5
Q
What is a molecule?
A
2 or more atoms chemically bonded together. (same or different)
6
Q
Define a compound.
A
Two or more atoms of DIFFERENT elements chemically bonded together.
7
Q
What is a mixture?
A
Two or more types of atoms, molecules, or compounds which AREN’T chemically bonded.
8
Q
Define an ion.
A
A positively or negatively charged atom.
9
Q
Define diatomic.
A
(to an element) An element/molecule which only occurs naturally in pairs.
10
Q
What is a covalent bond and how is it held together?
A
A bond in which non-metal atoms are held together by a shared pair of electrons that are attracted to the positive nuclei of the atoms.
11
Q
What is an ionic bond and how is it held together?
A
A bond between a metal and a non-metal, held together by oppositely charged ions.
12
Q
What is group 1 called?
A
Alkali Metals
13
Q
What is group 7 called?
A
The Halogens
14
Q
What is group 0 called?
A
Noble Gases
15
Q
What are the diatomic elements?
A
Iodine
Bromine
Chlorine
Fluorine
Nitrogen
Hydrogen
Oxygen
16
Q
How are ionic bonds formed?
A
When a metal donates its outer electrons to a non metal
17
Q
Do ionic substances conduct electricity and why?
A
Only when AQUEOUS (dissolved in water) or MOLTEN (melted)
This is because the ions are free to move.
18
Q
Why do covalent molecules have low boiling and melting points?
A
Because their INTERMOLECULAR FORCES are weak and break easily.
19
Q
How and why are ions formed?
A
Ions are formed when atoms lose or gain electrons in order to become stable.
20
Q
Define a diatomic element.
A
An element which only naturally exists as a pair.
21
Q
Why can graphite conduct but diamond can’t?
A
Graphite has delocalised electrons which move between layers, allowing electricity to flow.
22
Q
What charge is the nucleus of an atom?
A
Positive
23
Q
What are the four shapes of molecular bonds?
A
Linear
Angular
Trigonal Pyramidal
Tetrahedral
24
Q
What is formula mass?
A
The MASS of a CHEMICAL FORMULA.
25
How are elements arranged on the periodic table?
In order of INCREASING ATOMIC number
26
What are the horizontal rows on the periodic table called?
Periods
27
What are the vertical columns on the periodic table called?
Groups
28
What does it mean when elements are in the same atomic group?
They have SIMILAR CHEMICAL PROPERTIES
29
Where are the nonmetals located on the periodic table?
On the right side (after staircase)
30
Where are the METALS located on the periodic table?
On the left side (left of staircase)
31
What is all matter made up of?
Atoms
32
Define an element.
A SUBSTANCE that contains only ONE TYPE of atom
33
What particles are found in the nucleus?
Protons and Neutrons
34
Where are electrons located?
In the electron shells
35
What is the mass of an electron?
0 AMU
36
What is the mass of a proton?
1 AMU
37
What is the mass of a neutron?
1 AMU
38
What is the charge of a proton?
+1 (Positive)
39
What is the charge of a neutron?
0 (Neutral)
40
What is the charge of an electron?
-1 (Negative)
41
What is the atomic number?
The number of protons in an atom.
42
What is the mass number?
The number of Protons + Neutrons in an atom.
43
Why do atoms have no charge?
Atoms have no charge because they have equal amounts of protons and electrons, which balance each other.
44
Why do elements in the same group have similar properties?
Elements in the same group have similar properties because they have the same number of outer electrons in their outer shell.
45
How should you write electron arrangement?
PAGE 6 OF DATA BOOKLET
Going from innermost shell to outermost shell, in clockwise direction.
46
What is an isotope?
An isotope is an atom with the same atomic number as the original element but a different mass number.
TLDR; Same atomic number, varied mass number.
47
When going down a period on the periodic table, how is reactivity affected in METALS?
Reactivity INCREASES as you go down a group of METALS.
48
When going down a period on the periodic table, how is reactivity affected in NON-METALS?
Reactivity DECREASES as you go down a group of NON-METALS.
49
What is the reactivity of the noble gases?
They are inert/unreactive
50
What is the top number in nucleide notation?
MASS number
51
What is the bottom number in nucleide notation?
Atomic number
52
What should nucleide notation show?
Atomic Number
Mass Number
Charge
53
How do you calculate RAM (relative atomic mass)?
RAM =
(mass of isotope A x %) + (mass of isotope B x %)
-------------------------------------------------------
100
54
What does the suffix "-ide" mean?
2 element compound
55
What does the suffix "-ate" mean?
2 Elements + Oxygen (a lot)
56
What does the suffix "-ite" mean?
2 Elements + Oxygen (a little)
57
What are the exceptions to the "-ide"/"-ate" rule?
Magnesium Hydroxide = MgH2O2
Ammonium Chloride = ClH4
58
How can chemical formula be calculated?
SVSDF
59
How do calculate formula if prefixes are involved?
Ignore valency
60
What is a word equation?
An equation with the full names of each reactant and the products they form written out.
ie. Magnesium Oxide + Hydrogen --> Magnesium Hydroxide
61
What does the term aqueous mean?
Dissolved in water
62
What are roman numerals used for?
The valency of transition metals.
63
What does a chemical formula tell you?
The types of atoms in a molecule and how many there are of each.
64
What does the formula of a covalent network do?
It gives the simplest ratio of each atom in the network.
65
What is an ion?
A charged atom
66
How do you balance a chemical equation?
By changing the coefficients
67
Define a compound.
Two or more atoms of DIFFERENT elements which are chemically bonded together.
(A compound is a molecule)
68
What type of elements are covalent bonds between?
Non-metals and non-metals
69
What is a covalent bond?
A chemical bond formed when two or more atoms share electrons.
70
What holds covalent bonds together?
Covalent bonds are held together by two or more shared outer electrons and their attraction to the positive nuclei involved.
71
What is ionic bonding?
Transfer of electrons
72
Which elements form ionic bonds?
Metals and non-metals
73
Do metals give or take electrons in bonding?
Give/lose
74
Do non-metals give or take electrons?
Take/gain
75
What type of ion do metals form?
POSITIVE ions (+1)
76
What type of ions do non-metals make?
NEGATIVE ions (-1)
77
What holds an ionic bond together?
Electrostatic attraction between the positive and negative ions
78
What is a covalent network?
A very large structure of covalently bonded atoms.
Properties:
HIGH melting point
DOES NOT conduct electricity (excluding graphite)
79
Name 5 examples of covalent networks:
- Carbon (ONLY diamond and graphite)
- Boron
- Silicon
- Silicon Dioxide (Quartz)
- Silicon Carbide
80
How are carbons shaped in diamonds?
Tetrahedral shape
81
Name all of the diatomic elements.
BICHONF
Bromine
Iodine
Chlorine
Hydrogen
Oxygen
Nitrogen
Fluorine
82
Name all molecular shapes.
Linear
Angular
Pyramidal
Tetrahedral
83
What are intermolecular forces?
Intermolecular forces are the forces found in between molecules.
84
Describe the intermolecular forces of a covalent molecule.
Intermolecular forces between a covalent network are WEAK.
85
List the ways you can increase the rate of a reaction.
- Increase temperature
- Add a catalyst
- Increase the concentration of reactant
- Decrease in particle size/increase of surface area
86
Define a catalyst.
A catalyst is a substance which speeds up chemical reactions, but can be recovered while CHEMICALLY UNCHANGED at the end of a reaction.
87
How can you calculate the rate of reaction?
∆ Quantity / ∆ Time
88
How would you calculate the mass of a mole of any substance?
Gram Formula Mass (GFM)
89
How do you calculate GFM?
By adding up all of the RAMs inside the compound
90
What is the mass of 2 moles of NaCl?
GFM:
•Na- 1 x 23 = 23
•Cl- 1 x 35.5 = 35.5
GFM= 23 + 35.5 = 58.5g
Sub into Formula:
n=m/GFM
2= m/58.5
Solve:
m= 2 x 58.5
m= 117g
91
How can calculations be performed using the relationship between the mass and the number of moles in a substance?
N = m/GFM
N — Number of Moles
m — Mass
GFM — Gram Formula Mass
92
How can calculations be performed using the relationship between volume, concentration and number of moles in a substance?
N = cv (litres)
N — Number of Moles
c — Concentration
v — Volume
93
Calculate the volume of a 2 molL-1 solution containing 0.1 moles of solute
n=CV
V=n/C
V= 0.1/2
V=0.05L
94
Calculate the mass of 500 cm3 of a 2 molL-1 solution of K2CO3
GFM:
• K2- 2 x 39= 78
• C- 1 x 12= 12
• O3- 3 x 16= 48
•GFM=78+12+48= 138g
Sub into Formulae:
• C=2 n=? V= 500cm3= 0.5 LITRES
• n=? m=? GFM= 138g
Solve first equation:
n=CV
n= 2 x 0.5
n= 1 mole
Use info to solve second equation:
n=m/GFM
m= n x GFM
m= 1 x 138
m= 138g
95
Define solvent.
The SUBSTANCE that DISSOLVES the SOLUTE.
96
Define solute.
A solute is a substance dissolved in a solvent to create a solution.
97
Define solution.
The result of a solute dissolved in a solvent.
98
What is the pH scale?
An indication of the hydrogen ion concentration.
Runs from 0 to 14.
<7 acid
7= neutral
>7 alkaline
99
Name a feature of neutral solutions.
Have equal concentrations of H+(aq) and OHˉ(aq) ions.
100
Name the features of acids.
- HIGHER concentration of H+(aq) ions than OHˉ(aq) ions
- <7 pH
101
Describe the relationship between quantities of OHˉ ions and the periodic table.
As you go HIGHER in the periodic table (towards 14), the quantity of OHˉ ions INCREASES and H+ DECREASES.
102
Describe the relationship between quantities of H+ ions and the periodic table.
As you go LOWER in the periodic table (towards 0), the quantity of H+ ions INCREASES and OHˉ(aq) DECREASES.
103
Between two, what is the more common ion in ALKALIS?
Alkalis have a HIGHER concentration of OHˉ ions than H+ ions.
104
Between two, what is the more common ion in ACIDS?
Acids have a HIGHER concentration of H+ ios than OHˉ ions.
105
Name the features of alkalis.
- Higher concentration of OHˉ ions than H+ ions
- >7 pH
106
What is the equation for the disassociation of water?
H2O(l) <--> H+(aq) + OH-(aq)
107
What do all acids contain?
Hydrogen
108
What happens when you dilute an acid with water?
- pH INCREASES towards 7 (water is neutral)
- DECREASES the concentration of H+ (aq) ions.
109
What happens when you dilute an alkali with water?
- pH DECREASES towards 7
- DECREASES concentration of OHˉ (aq) ions.
110
What do SOLUBLE NON-METAL OXIDES form when dissolved in water?
ACIDIC solutions
111
What do SOLUBLE METAL OXIDES form when dissolved in water?
ALKALINE solutions.
112
State the equation for SOLUBLE METAL OXIDES dissolving in water?
Metal oxide + Water → Metal Hydroxide
113
Define a BASE.
A substance that reacts with an acid to make water.
114
List examples of bases.
- Metal Oxides
- Metal Hydroxides
- Metal Carbonates
- Ammonia
115
What do SOLUBLE BASES form when dissolved in water?
Alkaline solutions.
116
What is a neutralisation reaction?
A neutralisation reaction is a reaction in which a BASE reacts with an ACID to form WATER. One of the products is SALT.
117
State the equation for the neutralisation reaction of metal oxide.
Metal oxide + Acid → Salt + Water
118
State the equation for the neutralisation reaction of metal hydroxide.
Metal hydroxide + Acid → Salt + Water
119
State the equation for the neutralisation reaction of metal carbonate.
Metal carbonate + Acid → Salt + Water + Carbon dioxide
120
How are salts named?
Prefix — The NON-ACID
Suffix — The ACID NAME
121
Define a SPECTATOR ION.
A spectator ion is an ion that is present during the reaction but remains unchanged by the reaction.
122
State the neutralisation equation for magnesium reacting with hydrochloric acid.
Hydrochloric acid + Magnesium —> Magnesium chloride + water
HCl + Mg -> MgCl2 + H2O
123
How are carbons shaped in graphite?
in LAYERS of HEXAGONS.
124
What is the melting/boiling point of covalent networks and why?
Covalent networks have a very high melting and boiling point because their covalent bonds are strong and take a lot of energy to break.
125
What is the melting/boiling point of covalent compounds?
Very low because their covalent bonds are weak.
126
What is the melting/boiling point of ionic compounds?
Ionic compounds have a high melting and boiling point because they have strong intermolecular forces.
127
What state are ionic compounds in while at room temperature?
Solids.
128
Can covalent compounds conduct electricity?
No (except Graphite)
129
Can covalent networks conduct electricity?
No (excluding Graphite).
130
Can ionic compounds conduct electricity?
Only when in molten or aqueous state.
131
What state are covalent compounds at in room temperature?
Any.
132
Are covalent networks soluble?
No.
133
Are ionic compounds soluble in water?
Most, but not all, are.
134
Why can ionic compounds conduct electricity but only as aqueous or molten?
Molten or aqueous ionic compounds conduct electricity because the freely moving ions carry charge.
135
What is the formula for sulfuric acid?
H2SO4
136
What is the formula for nitric acid?
HNO3
137
Define titration.
Titration is a method in which a solution of KNOWN CONCENTRATION is used to determine the concentration of an UNKNOWN SOLUTION.
138
Metal Oxide + Acid —>
Salt + Water
139
Metal Hydroxide + Acid —>
Salt + Water
140
Metal Carbonate + Acid —>
Salt + Water + Carbon Dioxide
141
How are elements arranged in the periodic table?
In order of increasing atomic number.
