Chemistry Semester 1 Flashcards
(139 cards)
1
Q
describe the structure and behaviour of particles in liquid
A
the particles stay close together but are free to move, taking the shape of their container
2
Q
describe the structure and behaviour of particles in gases
A
particles spread out and move in a constant motion
3
Q
what is reduction
A
losing oxygen or gaining electrons
4
Q
how do you calculate the molarity
A
molarity = number of moles of solute / volume solution in litres
5
Q
what charge are protons
A
positive
6
Q
describe the behaviour of the valence electrons in a molecular covalent bond
A
the electrons are shared
7
Q
what charge will sodium have when it forms ions
A
1+
8
Q
describe the behaviour of the valence electrons in a covalent network
A
electrons are shared
9
Q
what is an ion
A
an atom that has gained or lost electrons
10
Q
where are protons found in an atom
A
in the nucleus
11
Q
what is a combustion reaction
A
element or compound reacts with oxygen, often with the release of energy in the form of light and heat
12
Q
what is non polar covalent bonding
A
when two atoms share a pair of electrons with each other evenly
13
Q
what ion does silver usually create
A
1+
14
Q
what charge are metals
A
positive
15
Q
what are alkaline earth metals
A
higher density than alkali metals and not as soft as alkali metals, reactive but not as much alkali metals, form alkaline solutions when combined with water
16
Q
what is deposition
A
a gas to a solid
17
Q
describe the electrodes in a simple cell
A
anode (site of oxidation) (negative charge), cathode (site of reduction) (positive charge)
18
Q
where are the transition metals located on the periodic table
A
in the middle section
19
Q
how do you figure out the number of neutrons in an atom
A
atomic mass - protons
20
Q
what are alkali metals
A
low-density soft metals, extremely reactive, form alkaline solutions when combined with water
21
Q
describe the typical physical properties of substances with metallic bonds
A
- high melting and boiling point
- excellent conductors of electricity
- malleable
- shiny
22
Q
what type of bond forms between a non-metal and another non-metal
A
covalent bonding
23
Q
what is a decomposition reaction
A
one reactant breaks down to form two or more products (AB —> A + B)
24
Q
describe the general shape or structure of the particles involved in a metallic bond
A
each metal atom is surrounded by lots of other metal atoms, and they all share their valence electrons
25
what is a monatomic element
when there is one atom and one molecule
26
what are noble gases
all are gases at room temperature and are monatomic. These are highly unreactive and do not readily combine with other elements.
27
what does the period number tell you
how many electron shells the element has
28
where are the halogens located in the periodic table
in the second last column
29
what are 3 tests that could be done to determine whether a substance is a metal or not
1. Stress test (hit it with a hammer) – if it bends – it is likely to be a metal
2. Electrical conductivity test – if it conducts – it is likely to be a metal
3. Scratch / cut test – if it is shiny (metallic lustre) – it is likely to be a metal
30
what are halogens
generally, gases are at room temperature or at least have low melting points and boiling points. All are highly reactive and readily “grab” valence electrons
31
how do you calculate the number of moles
number of moles = mass of substance / mass of one mole
32
what is the charge of a beryllium ion
2+
33
what charge will chlorine have when it forms ions
1-
34
what are the columns in the periodic table called
groups
35
what is the opposite of deposition
sublimation
36
what charge will beryllium have when it forms ions
2+
37
how do you figure out the empirical formula
the lowest relative ratios of different atoms in a compound
38
what is the opposite of condensation
evaporation
39
how do we know if a covalent bond is polar
if the difference between both electron negativities is greater than 0.3 and smaller than 1.7
40
what is a combination reaction
two or more reactants combining to form one product (A + B ---> AB)
41
what is the purpose of a simple cell
to produce an electrical current
42
what is the relative molecular mass
the weight in grams of the number of atoms of the element contained in 12.00 g of carbon-12
43
list 3 or more properties of metals
- high melting and boiling points
- good conductors of electricity
- good conductors of heat
- high density
- malleable
- ductile
- sonorous
44
which atomic particles are involved in all bonding
valence electrons
45
what charge are electrons
negative
46
what are two substances that must be present for the rusting of iron to occur
oxygen and water
47
describe the typical physical properties of substances with molecular covalent bonding
- low melting and boiling point
- poor conductors of electricity
- soft
48
what is a double-replacement reaction
exchange of positive ions between two ionic compounds (AB + CD ---> AC + BD)
49
what are valence electrons
electrons located in the outermost shell
50
describe the electrodes in a electrolytic cell
anode (site of oxidation) (positive charge), cathode (side of reduction) (negative charge)
51
what is the number of particles (or molecules) in one mole of any substance
6.02 x 10^23
52
what are the rows on the periodic table
periods
53
how do you figure out the number of protons in an atom
the atomic number
54
what is a chemical change
when a new substance is formed and its not easy to reverse
55
what is the charge of a fluoride ion
1-
56
what type of bonds form between a metal and a non metal
iconic bonding
57
describe the electrolyte in an electrolytic cell
usually reduction ion and allows ion movement
58
where are electrons found in an atom
they are grouped around the nucleus into shells
59
what is oxidation
gaining oxygen or losing electrons
60
where are the alkali metals located in the periodic table
in the first column
61
what charge are neutrons
neutral/no charge
62
describe the typical physical properties of substances with ionic bonding
- high melting and boiling point
- poor conductors of electricity when solids
- good conductors of electricity when liquid or dissolved
- hard and brittle
63
what are transition metals
generally hard and higher density than Group 1 and 2 metals, many form different coloured solutions in ion form, some are magnetic
64
describe the behaviour of the valence electrons in an ionic bond
the electrons are lost and gained
65
what type of bonding is it when the electronegativity difference is greater than 1.7
iconic
66
how do you determine if a reaction is precipitate or not
Determine the possible products using the double displacement equation. Then predict whether either of the possible products is insoluble using the solubility chart. If one is insoluble it will form a precipitate
67
what is an isotope
an element with more or less neutrons
68
what is reduction
the loss of oxygen and gain of electrons
69
what is the purpose of an electrolytic cell
use electrical current to drive reaction
70
how do you calculate the percentage composition of an element in a compound
(total molar mass of just the element / molar mass of the whole compound) x 100%
71
describe the electrolyte in a simple cell
usually an acid and allows ion movement
72
what is an ionic bond
valence electrons are lost (metals) or gained (non-metals). Occurs between metal and non-metal
73
where are neutrons found in an atom
in the nucleus
74
list 3 or more properties of non metals
- poor conductors of heat and electricity
- dull in their appearance
- weak and brittle
- generally low melting and boiling points, meaning they are gases and liquids at room temperature
- not sonorous
75
what is oxidation
the gain of oxygen or the loss of electrons
76
where are the alkaline earth metals located on the periodic table
in the second column
77
what does the group number tell you
how many electrons are in the valence shell
78
what is a diatomic element
when there are two atoms and one molecule
79
what does a "two-way" arrow indicate?
that a reaction is reversible
80
describe the motion of particles with increasing temperature
when the temperature increases, the kinetic energy also increases
81
what is a metallic bond
valence electrons form a “sea of electrons” around positively charged cations. Occurs between metal and metal atoms
82
what is polar covalent bonding
when the shared electrons are not shared evenly and have different electronegativities. This results in a slightly positively charged end of the molecule and a slightly negatively charged end of the molecule.
83
what is a single-replacement reaction
atoms of one element replace the atoms of another element in a compound (A + BC ---> AC + B)
84
describe the typical physical properties of substances with covalent networks
- high melting and boiling point
- poor conductors of electricity
- hard and brittle
85
how do you calculate the formula mass of a compound
adding the masses of each individual atom in the formula of the compound
86
why does a solid ionic compound not conduct electricity yet a salt solution conducts electricity very well
In the solid state, the ionic compounds do not conduct electricity because, in a solid, the positive and negative ions are locked in position and therefore cannot conduct. However, when put in water, the ionic compounds are broken apart by water molecules ions and the positive and negative ions are free to move hence these ions are responsible for the conduction of electricity.
87
what ion does zinc usually create
2+
88
what is condensation
a gas to a liquid
89
what is a physical change
when no new substance is formed and it is usually easy to reverse
90
what is a covalent bond
valence electrons are shared. Occurs between non-metal and non-metal
91
Do covalent compounds conduct electricity
their electrical conductivity is generally quite poor, whether in the solid or liquid state.
92
what is an allotrope
the same element in a different physical form resulting in very different substances
93
describe the general shape or structure of the particles involved in a covalent network
large, rigid three-dimensional arrangements of atoms held together by strong covalent bonds
94
describe the structure and behaviour of particles in solids
the particles are close together and vibrate a little in fixed positions
95
what does it mean for a metal to be malleable
metals that tend to bend when put under stress
96
what type of bonds form between a metal and another metal
metallic bonding
97
describe the behaviour of the valence electrons in a metallic bond
valence electrons continually move from one atom to another and are not associated with any specific pair of atoms
98
what is a redox reaction
reactions that involve the transfer of electrons from one species to another
99
describe the general shape or structure of the particles involved in an ionic bond
lattice structure with regular repeating arrangement of metal and non metal ions
100
what is a precipitate reaction
A solid produced by reaction between two clear solutions is called a precipitate
101
what charge will phosphorus have when it forms ions
3-
102
where are the noble gases located in the periodic table
in the last column
103
what charge will oxygen have when it forms ions
2-
104
describe the general shape or structure of the particles involved in a molecular covalent bond
discrete molecules - small groups of atoms held together by strong covalent bonds inside the molecule and weak intermolcular forces between the molecules.
105
what is a mole
the quantity which contains as many elementary units as there are atoms in exactly 12 grams of the carbon-12 isotope.
106
what is the Avogadro constant
number of atoms in exactly 12 grams of the carbon-12 isotope (6.02 × 10^23)
107
what is the mole of an element
atomic weight
108
what is the mole of a compound
molecular weight
109
what are other names for molecular weight
molar mass, molecular mass, formula weight, formula mass,
110
how do you find the number of atoms or molecules
number of moles x Avogadro constant (6.02 x 10^23)
110
how do you find the number of atoms or molecules
number of moles x Avogadro constant (6.02 x 10^23)
111
what does a chemical equation tell us
the ratio by mass in which substances react or are formed in a reaction
112
what is a saturated solution
when no more of the particular solute can be dissolved in a given quantity of the solvent at the specified temperature
113
what is an unsaturated solution
a solution that contains less than this maximum amount of solute
114
what is the solubility of a substance in a particular solvent
the concentration of its saturated solution at the specified temperature. It is the maximum amount of the substance that will dissolve in a given amount of the solvent at that temperature
115
what is molarity
number of moles of solute per litre of solution
116
what are other names for a simple cell
electrochemical cell, electric cell, voltaic cell
117
how are simple cell made
when two different metals are placed in a conducting solution and connected together
118
what is the conducting solution in a simple cell called
electrolyte
119
what is the metal strips in a simple cell called
electrodes
120
what are dry cells
when liquid electrolyte has been replace with a moist electrolyte paste in a sealed container
121
what is electroplating
putting a layer of metal on the surface of another metal
122
what is corrosion
a reaction between a metal and moist air
123
what is an anion
negatively charged ion
124
what is a cation
a positively charged ion
125
what is an ionic compound
transfer of electrons from 1 atom to another. consists of electrostatic attraction between positive (metal, cation) and negative (non-metal, anion) ions formed by the transfer of electrons
126
what is a covalent bond
formed between pairs of atoms by sharing electrons which form covalent bonds/molecular bonds/compound (non metal to non metal)
127
what are polyatomic ions
covalent bonds that have a charge
128
what are the properties of an ionic bond
- high melting and boiling point - needs a lot of energy to break apart bonds
- hard but britle
- as solids do not conduct electricity
- as liquid, molten or aqueous solution conducts electricity because ions are separated and have charges that can move
129
what are the properties of a covalent bond
- low melting and boiling point - don't need as much energy because it has weak IMF (intermolecular force)
- soft at solid-state - only weak IMF are broken when squashed
- pure - does not conduct electricity
- as an aqueous solution, does not conduct unless water forms ions
- has no charges that can move
130
what is electronegativity
the amount of attraction an element has for electrons. The higher the number the high the attraction
131
what is the current
amount of electrons flowing
132
what is the unit for currents
amps (A) - amount of electrons per second
133
what is the voltage
amount of energy available to electrons. amount of "push" electrons have. potential difference between 2 points on a circuit
134
what is the unit for voltage
volts (V)
135
what is a lattice
an indefinite orderly array of particles
136
what are the diatomic elements
Hydrogen (H2), Nitrogen (N2), Oxygen (O2), Fluorine (F2), Chlorine (Cl2), Iodine (I2), Bromine (Br2)
137
how do you name covalent compounds
using the prefix system
138
how do you namet ionic compounds
using the stock system (roman numerals)
