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Chemistry > Chemistry Semester 1 > Flashcards

Chemistry Semester 1 Flashcards

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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

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2
Q

describe the structure and behaviour of particles in gases

A

particles spread out and move in a constant motion

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3
Q

what is reduction

A

losing oxygen or gaining electrons

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4
Q

how do you calculate the molarity

A

molarity = number of moles of solute / volume solution in litres

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5
Q

what charge are protons

A

positive

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6
Q

describe the behaviour of the valence electrons in a molecular covalent bond

A

the electrons are shared

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7
Q

what charge will sodium have when it forms ions

A

1+

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8
Q

describe the behaviour of the valence electrons in a covalent network

A

electrons are shared

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9
Q

what is an ion

A

an atom that has gained or lost electrons

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10
Q

where are protons found in an atom

A

in the nucleus

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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

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12
Q

what is non polar covalent bonding

A

when two atoms share a pair of electrons with each other evenly

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13
Q

what ion does silver usually create

A

1+

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14
Q

what charge are metals

A

positive

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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

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16
Q

what is deposition

A

a gas to a solid

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17
Q

describe the electrodes in a simple cell

A

anode (site of oxidation) (negative charge), cathode (site of reduction) (positive charge)

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18
Q

where are the transition metals located on the periodic table

A

in the middle section

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19
Q

how do you figure out the number of neutrons in an atom

A

atomic mass - protons

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20
Q

what are alkali metals

A

low-density soft metals, extremely reactive, form alkaline solutions when combined with water

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21
Q

describe the typical physical properties of substances with metallic bonds

A
  • high melting and boiling point
  • excellent conductors of electricity
  • malleable
  • shiny
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22
Q

what type of bond forms between a non-metal and another non-metal

A

covalent bonding

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23
Q

what is a decomposition reaction

A

one reactant breaks down to form two or more products (AB —> A + B)

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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

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25
Q

what is a monatomic element

A

when there is one atom and one molecule

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26
Q

what are noble gases

A

all are gases at room temperature and are monatomic. These are highly unreactive and do not readily combine with other elements.

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27
Q

what does the period number tell you

A

how many electron shells the element has

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28
Q

where are the halogens located in the periodic table

A

in the second last column

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29
Q

what are 3 tests that could be done to determine whether a substance is a metal or not

A
  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
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30
Q

what are halogens

A

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

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31
Q

how do you calculate the number of moles

A

number of moles = mass of substance / mass of one mole

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32
Q

what is the charge of a beryllium ion

A

2+

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33
Q

what charge will chlorine have when it forms ions

A

1-

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34
Q

what are the columns in the periodic table called

A

groups

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35
Q

what is the opposite of deposition

A

sublimation

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36
Q

what charge will beryllium have when it forms ions

A

2+

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37
Q

how do you figure out the empirical formula

A

the lowest relative ratios of different atoms in a compound

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38
Q

what is the opposite of condensation

A

evaporation

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39
Q

how do we know if a covalent bond is polar

A

if the difference between both electron negativities is greater than 0.3 and smaller than 1.7

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40
Q

what is a combination reaction

A

two or more reactants combining to form one product (A + B —> AB)

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41
Q

what is the purpose of a simple cell

A

to produce an electrical current

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42
Q

what is the relative molecular mass

A

the weight in grams of the number of atoms of the element contained in 12.00 g of carbon-12

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43
Q

list 3 or more properties of metals

A
  • high melting and boiling points
  • good conductors of electricity
  • good conductors of heat
  • high density
  • malleable
  • ductile
  • sonorous
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44
Q

which atomic particles are involved in all bonding

A

valence electrons

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45
Q

what charge are electrons

A

negative

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46
Q

what are two substances that must be present for the rusting of iron to occur

A

oxygen and water

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47
Q

describe the typical physical properties of substances with molecular covalent bonding

A
  • low melting and boiling point
  • poor conductors of electricity
  • soft
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48
Q

what is a double-replacement reaction

A

exchange of positive ions between two ionic compounds (AB + CD —> AC + BD)

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49
Q

what are valence electrons

A

electrons located in the outermost shell

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50
Q

describe the electrodes in a electrolytic cell

A

anode (site of oxidation) (positive charge), cathode (side of reduction) (negative charge)

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51
Q

what is the number of particles (or molecules) in one mole of any substance

A

6.02 x 10^23

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52
Q

what are the rows on the periodic table

A

periods

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53
Q

how do you figure out the number of protons in an atom

A

the atomic number

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54
Q

what is a chemical change

A

when a new substance is formed and its not easy to reverse

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55
Q

what is the charge of a fluoride ion

A

1-

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56
Q

what type of bonds form between a metal and a non metal

A

iconic bonding

57
Q

describe the electrolyte in an electrolytic cell

A

usually reduction ion and allows ion movement

58
Q

where are electrons found in an atom

A

they are grouped around the nucleus into shells

59
Q

what is oxidation

A

gaining oxygen or losing electrons

60
Q

where are the alkali metals located in the periodic table

A

in the first column

61
Q

what charge are neutrons

A

neutral/no charge

62
Q

describe the typical physical properties of substances with ionic bonding

A
  • high melting and boiling point
  • poor conductors of electricity when solids
  • good conductors of electricity when liquid or dissolved
  • hard and brittle
63
Q

what are transition metals

A

generally hard and higher density than Group 1 and 2 metals, many form different coloured solutions in ion form, some are magnetic

64
Q

describe the behaviour of the valence electrons in an ionic bond

A

the electrons are lost and gained

65
Q

what type of bonding is it when the electronegativity difference is greater than 1.7

A

iconic

66
Q

how do you determine if a reaction is precipitate or not

A

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
Q

what is an isotope

A

an element with more or less neutrons

68
Q

what is reduction

A

the loss of oxygen and gain of electrons

69
Q

what is the purpose of an electrolytic cell

A

use electrical current to drive reaction

70
Q

how do you calculate the percentage composition of an element in a compound

A

(total molar mass of just the element / molar mass of the whole compound) x 100%

71
Q

describe the electrolyte in a simple cell

A

usually an acid and allows ion movement

72
Q

what is an ionic bond

A

valence electrons are lost (metals) or gained (non-metals). Occurs between metal and non-metal

73
Q

where are neutrons found in an atom

A

in the nucleus

74
Q

list 3 or more properties of non metals

A
  • 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
Q

what is oxidation

A

the gain of oxygen or the loss of electrons

76
Q

where are the alkaline earth metals located on the periodic table

A

in the second column

77
Q

what does the group number tell you

A

how many electrons are in the valence shell

78
Q

what is a diatomic element

A

when there are two atoms and one molecule

79
Q

what does a “two-way” arrow indicate?

A

that a reaction is reversible

80
Q

describe the motion of particles with increasing temperature

A

when the temperature increases, the kinetic energy also increases

81
Q

what is a metallic bond

A

valence electrons form a “sea of electrons” around positively charged cations. Occurs between metal and metal atoms

82
Q

what is polar covalent bonding

A

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
Q

what is a single-replacement reaction

A

atoms of one element replace the atoms of another element in a compound (A + BC —> AC + B)

84
Q

describe the typical physical properties of substances with covalent networks

A
  • high melting and boiling point
  • poor conductors of electricity
  • hard and brittle
85
Q

how do you calculate the formula mass of a compound

A

adding the masses of each individual atom in the formula of the compound

86
Q

why does a solid ionic compound not conduct electricity yet a salt solution conducts electricity very well

A

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
Q

what ion does zinc usually create

A

2+

88
Q

what is condensation

A

a gas to a liquid

89
Q

what is a physical change

A

when no new substance is formed and it is usually easy to reverse

90
Q

what is a covalent bond

A

valence electrons are shared. Occurs between non-metal and non-metal

91
Q

Do covalent compounds conduct electricity

A

their electrical conductivity is generally quite poor, whether in the solid or liquid state.

92
Q

what is an allotrope

A

the same element in a different physical form resulting in very different substances

93
Q

describe the general shape or structure of the particles involved in a covalent network

A

large, rigid three-dimensional arrangements of atoms held together by strong covalent bonds

94
Q

describe the structure and behaviour of particles in solids

A

the particles are close together and vibrate a little in fixed positions

95
Q

what does it mean for a metal to be malleable

A

metals that tend to bend when put under stress

96
Q

what type of bonds form between a metal and another metal

A

metallic bonding

97
Q

describe the behaviour of the valence electrons in a metallic bond

A

valence electrons continually move from one atom to another and are not associated with any specific pair of atoms

98
Q

what is a redox reaction

A

reactions that involve the transfer of electrons from one species to another

99
Q

describe the general shape or structure of the particles involved in an ionic bond

A

lattice structure with regular repeating arrangement of metal and non metal ions

100
Q

what is a precipitate reaction

A

A solid produced by reaction between two clear solutions is called a precipitate

101
Q

what charge will phosphorus have when it forms ions

A

3-

102
Q

where are the noble gases located in the periodic table

A

in the last column

103
Q

what charge will oxygen have when it forms ions

A

2-

104
Q

describe the general shape or structure of the particles involved in a molecular covalent bond

A

discrete molecules - small groups of atoms held together by strong covalent bonds inside the molecule and weak intermolcular forces between the molecules.

105
Q

what is a mole

A

the quantity which contains as many elementary units as there are atoms in exactly 12 grams of the carbon-12 isotope.

106
Q

what is the Avogadro constant

A

number of atoms in exactly 12 grams of the carbon-12 isotope (6.02 × 10^23)

107
Q

what is the mole of an element

A

atomic weight

108
Q

what is the mole of a compound

A

molecular weight

109
Q

what are other names for molecular weight

A

molar mass, molecular mass, formula weight, formula mass,

110
Q

how do you find the number of atoms or molecules

A

number of moles x Avogadro constant (6.02 x 10^23)

110
Q

how do you find the number of atoms or molecules

A

number of moles x Avogadro constant (6.02 x 10^23)

111
Q

what does a chemical equation tell us

A

the ratio by mass in which substances react or are formed in a reaction

112
Q

what is a saturated solution

A

when no more of the particular solute can be dissolved in a given quantity of the solvent at the specified temperature

113
Q

what is an unsaturated solution

A

a solution that contains less than this maximum amount of solute

114
Q

what is the solubility of a substance in a particular solvent

A

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
Q

what is molarity

A

number of moles of solute per litre of solution

116
Q

what are other names for a simple cell

A

electrochemical cell, electric cell, voltaic cell

117
Q

how are simple cell made

A

when two different metals are placed in a conducting solution and connected together

118
Q

what is the conducting solution in a simple cell called

A

electrolyte

119
Q

what is the metal strips in a simple cell called

A

electrodes

120
Q

what are dry cells

A

when liquid electrolyte has been replace with a moist electrolyte paste in a sealed container

121
Q

what is electroplating

A

putting a layer of metal on the surface of another metal

122
Q

what is corrosion

A

a reaction between a metal and moist air

123
Q

what is an anion

A

negatively charged ion

124
Q

what is a cation

A

a positively charged ion

125
Q

what is an ionic compound

A

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
Q

what is a covalent bond

A

formed between pairs of atoms by sharing electrons which form covalent bonds/molecular bonds/compound (non metal to non metal)

127
Q

what are polyatomic ions

A

covalent bonds that have a charge

128
Q

what are the properties of an ionic bond

A
  • 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
Q

what are the properties of a covalent bond

A
  • 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
Q

what is electronegativity

A

the amount of attraction an element has for electrons. The higher the number the high the attraction

131
Q

what is the current

A

amount of electrons flowing

132
Q

what is the unit for currents

A

amps (A) - amount of electrons per second

133
Q

what is the voltage

A

amount of energy available to electrons. amount of “push” electrons have. potential difference between 2 points on a circuit

134
Q

what is the unit for voltage

A

volts (V)

135
Q

what is a lattice

A

an indefinite orderly array of particles

136
Q

what are the diatomic elements

A

Hydrogen (H2), Nitrogen (N2), Oxygen (O2), Fluorine (F2), Chlorine (Cl2), Iodine (I2), Bromine (Br2)

137
Q

how do you name covalent compounds

A

using the prefix system

138
Q

how do you namet ionic compounds

A

using the stock system (roman numerals)

Chemistry (1 decks)

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