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Grade 11 Chemistry > Unit 1 Test Notes > Flashcards

Unit 1 Test Notes Flashcards

1
Q

What is the smallest possible particle of an element?

A

An atom

Atoms are the fundamental building blocks of matter.

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2
Q

What is a stable octet?

A

A full shell of eight electrons in the outer energy level of an atom

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3
Q

How do metal atoms in Groups 1, 2, or 3 achieve a stable octet?

A

They lose electrons to form cations

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4
Q

How do non-metal atoms in Groups 15, 16, or 17 achieve a stable octet?

A

They gain electrons to form anions

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5
Q

What are cations?

A

Positively charged ions that have lost electrons

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6
Q

What are anions?

A

Negatively charged ions that have gained electrons

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7
Q

What is the atomic number (Z)?

A

The number of protons in one atom of a specific element

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8
Q

What is atomic mass?

A

The average mass of an element, expressed in atomic mass units (amu)

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9
Q

How is atomic mass calculated?

A

of protons + # of neutrons

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10
Q

What are the charges of protons, electrons, and neutrons?

A
  • Proton: 1+
  • Electron: 1-
  • Neutron: 0
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11
Q

What does an isotope represent?

A

Atoms with the same number of protons but a different number of neutrons

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12
Q

What is isotopic abundance?

A

The percentage of a given isotope in a sample of an element

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13
Q

Fill in the blank: Atomic mass is a _______ average of all the isotopes of the element.

A

weighted

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14
Q

True or False: All isotopes of an element have the same atomic mass.

A

False

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15
Q

What is a mass spectrometer used for?

A

To determine the relative abundance of each isotope

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16
Q

What are the three types of particles emitted by radioisotopes?

A
  • Alpha particles
  • Beta particles
  • Gamma rays
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17
Q

How do you calculate the atomic mass given isotopic abundance?

A

atomic mass = (% abundance of isotope 1)(mass of isotope 1) + (% abundance of isotope 2)(mass of isotope 2)

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18
Q

What happens during the decay of a radioisotope?

A

It spontaneously produces two or more smaller nuclei and radiation

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19
Q

What are noble gases known for?

A

They are stable and inert because they have a stable octet

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20
Q

How is the atomic mass expressed?

A

In decimals

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21
Q

Who proposed that all matter can be divided into smaller pieces until a single indivisible particle is reached?

A

Democritus

Democritus introduced the concept of the atom, meaning ‘cannot be cut’.

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22
Q

What are the three key characteristics of atoms proposed by Democritus?

A
  • Atoms are of different sizes
  • Atoms are in constant motion
  • Atoms are separated by empty spaces
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23
Q

Which elements did Aristotle and Empedocles believe all matter was composed of?

A
  • Earth
  • Air
  • Fire
  • Water
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24
Q

What does Dalton’s theory state about atoms?

A
  • Matter consists of definite particles called atoms
  • Atoms cannot be created, destroyed, or divided
  • Each element has its own type of atom
  • Atoms of the same element have identical properties
  • Atoms can combine in constant ratios to form new substances
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25
Q

What is the ‘Plum Pudding Model’ proposed by Thomson?

A

A model where positive and negative charges are evenly spread throughout the atom.

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26
Q

What was the main finding of Rutherford’s gold foil experiment?

A

The atom is mostly empty space with a tiny, dense nucleus.

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27
Q

What is the role of protons in an atom?

A

Protons determine the identity of the element.

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28
Q

What did Bohr’s experiments with hydrogen atoms reveal?

A

Electrons exist in specific energy levels and emit light when they transition between these levels.

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29
Q

What are isotopes?

A

Atoms with the same number of protons but a different number of neutrons.

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30
Q

Fill in the blank: Matter is anything that has mass and takes up _______.

A

space

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31
Q

What is the definition of an element?

A

A pure substance that cannot be broken down into simpler substances by any physical or chemical means.

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32
Q

What is a compound?

A

A pure substance composed of two or more different elements that are chemically joined.

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33
Q

What does IUPAC stand for?

A

International Union of Pure and Applied Chemistry

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34
Q

Who proposed using a code of letters as symbols for elements?

A

Jons Jakob Berzelius

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35
Q

True or False: Alchemy was a time of intense exploration of the nature of matter.

A

True

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36
Q

What is empirical knowledge?

A

Knowledge that comes from investigation and observation.

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37
Q

What is theoretical knowledge?

A

Knowledge that explains scientific observations.

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38
Q

Fill in the blank: A _______ is an explanation or model that depends on observation, experimentation, and reasoning.

A

theory

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39
Q

What are the two main types of knowledge in scientific research?

A
  • Empirical Knowledge
  • Theoretical Knowledge
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40
Q

What is the modern model used by physicists and chemists to describe electrons?

A

Quantum Mechanical Model

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41
Q

What is the significance of the periodic table?

A

Each element has its own square containing the element symbol, atomic number, and atomic mass.

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42
Q

What information is contained in each square of the periodic table?

A

Element symbol, atomic number, atomic mass

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43
Q

In what year were 31 elements known?

A

1800

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44
Q

Who proposed the law of triads?

A

Johann Dobereiner

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45
Q

What does the law of triads state?

A

The middle element has an atomic mass about halfway between the other two

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46
Q

What pattern did John Alexander Newlands observe?

A

Similar chemical and physical properties appeared for every 8th element

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47
Q

What is the law of octaves?

A

The observation that every 8th element has similar properties

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48
Q

Who published the first periodic law?

A

Dmitri Mendeleev

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49
Q

What did Mendeleev do with the elements in his periodic table?

A

Listed them in horizontal rows by atomic mass and grouped similar properties

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50
Q

What are the two main classifications of rows and columns in the periodic table?

A

Rows are called periods, and columns are called groups or chemical families

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51
Q

What do elements in the same group share?

A

Certain physical and chemical properties

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52
Q

What are the characteristics of Group 1 elements?

A

Soft, silver-coloured, very reactive metals with 1 valence electron

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53
Q

Fill in the blank: Group 2 elements are known as _______.

A

Alkaline Earth Metals

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54
Q

What are the properties of Group 17 elements?

A

May be solids, liquids, or gases; extremely reactive; 7 valence electrons

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55
Q

What are the characteristics of Noble Gases in Group 18?

A

Gases at SATP, extremely unreactive, full outer shell

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56
Q

What three classes can elements be divided into based on properties?

A
  • Metals
  • Non-Metals
  • Metalloids
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57
Q

What are the characteristics of metals?

A

Most are solid at SATP, shiny, excellent conductors, malleable, ductile

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58
Q

How many non-metals are there, and what are their states at room temperature?

A

17 non-metals: 11 gases, 5 solids, 1 liquid

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59
Q

What are metalloids?

A

Elements with metallic and non-metallic properties, semi-conductors, brittle solids

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60
Q

What are Bohr-Rutherford diagrams used for?

A

To show the subatomic particles in an atom

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61
Q

What do chemical reactions involve in an atom?

A

Valence electrons in the valence shell

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62
Q

How many electrons can each orbital hold?

A
  • Orbital #1: 2 electrons
  • Orbital #2: 8 electrons
  • Orbital #3: 8 electrons
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63
Q

What do Lewis Dot diagrams represent?

A

Valence electrons

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64
Q

How many valence electrons does Oxygen have?

A

6 valence electrons

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65
Q

What are lone pairs in the context of Lewis Dot diagrams?

A

Electrons that are by themselves

66
Q

What is a trend in the context of the periodic table?

A

A predictable change in a particular direction

67
Q

What happens to atomic radius as you move across a period?

A

Decreases

68
Q

What is the atomic radius?

A

A measurement of the size of an atom, usually expressed in picometres (pm)

69
Q

What causes the atomic radius to decrease across a period?

A

Increased nuclear charge with no additional shielding

70
Q

What happens to atomic radius as you move down a group?

A

Increases

71
Q

What is the effective nuclear charge (ENC)?

A

The charge felt by valence electrons after accounting for shielding electrons

72
Q

What is the relationship between positive ions and atomic radius?

A

Positive ions have a smaller radius than the neutral atom from which they are formed

73
Q

What is ionization energy?

A

The quantity of energy required to remove a single valence electron from an atom or ion in a gaseous state

74
Q

How does ionization energy change across a period?

A

Tends to increase

75
Q

How does ionization energy change down a group?

A

Tends to decrease

76
Q

What is electron affinity?

A

The energy change that occurs when an electron is added to a neutral atom in a gaseous state

77
Q

How does electron affinity change across a period?

A

Increases

78
Q

How does electron affinity change down a group?

A

Decreases

79
Q

What is electronegativity?

A

The ability of an atom or molecule to attract pairs of electrons in a chemical bond

80
Q

Which element is the most electronegative?

A

Fluorine

81
Q

Fill in the blank: The outermost electrons are lost when an atom forms a _______.

A

Positive ion or cation

82
Q

Fill in the blank: The addition of an electron from an atom results in the formation of a _______.

A

Negative ion or anion

83
Q

True or False: Electronegativity decreases as you move across a period.

A

False

84
Q

What is the first ionization energy?

A

The amount of energy required to remove the most weakly held electron from a neutral atom

85
Q

What is the second ionization energy?

A

The amount of energy required to remove a second electron from a positive ion

86
Q

What role does electron shielding play in atomic structure?

A

It decreases the effective nuclear charge felt by outer electrons

87
Q

How does the number of energy levels affect atomic radius?

A

More energy levels increase atomic radius due to increased shielding

88
Q

What happens to the electron cloud when an atom gains an electron?

A

It increases, leading to greater electron-electron repulsion

89
Q

What is a chemical bond?

A

Forces of attraction holding atoms or ions together.

90
Q

What is an ionic compound?

A

A pure substance formed from a metal and a non-metal composed of oppositely charged ions.

91
Q

What happens to sodium and chlorine when they form an ionic bond?

A

Sodium loses a valence electron to form a cation, and chlorine accepts the electron to form an anion.

92
Q

What is a molecular compound?

A

A pure substance formed from two or more different non-metals sharing electrons.

93
Q

What are the properties of ionic compounds?

A

• Solids at SATP
• High melting point
• Neutral compounds
• Electrolytes

94
Q

What is the reason for the high melting point of ionic compounds?

A

Ions are held together by strong electrostatic forces (ionic bonds).

95
Q

What is an electrolyte?

A

A substance that forms a solution that conducts electricity.

96
Q

What is the structure of ionic compounds known as?

A

Crystal lattice.

97
Q

What does the arrangement of cations and anions in an ionic compound explain?

A

Why these substances are hard and brittle.

98
Q

What is the smallest repeating unit in an ionic crystal structure called?

A

Formula unit.

99
Q

What is the formula unit of potassium sulfide (K2S)?

A

2:1 ratio of potassium ions to sulfide ion.

100
Q

What is a stable octet?

A

A full shell of eight electrons in the outer energy level of an atom.

101
Q

How do metal atoms in Groups 1, 2, or 3 achieve a stable octet?

A

By losing electrons to form cations.

102
Q

How do non-metal atoms in Groups 15, 16, or 17 achieve a stable octet?

A

By gaining electrons to form anions.

103
Q

What are electron dot diagrams or Lewis symbols?

A

A representation of an atom or ion, made up of the chemical symbol and dots indicating the number of electrons in the valence energy level.

104
Q

True or False: Noble gases are reactive because they have a stable octet.

A

False.

105
Q

Fill in the blank: The electrostatic force between the cation and anion holds these ions together, forming an _______.

A

ionic bond.

106
Q

What is the significance of water molecules in ionic compounds?

A

They surround each ion and separate it from the crystal, allowing ions to move and carry electric charges.

107
Q

What is a molecular compound?

A

A pure substance formed from two or more different non-metals

Examples include water (H2O) and carbon dioxide (CO2)

108
Q

Define a molecular element.

A

A pure substance composed of molecules made up of two or more atoms of the same element

Examples include O2, N2, and Cl2.

109
Q

What is a diatomic molecule?

A

A molecule consisting of two atoms of the same or different elements

110
Q

What is a polyatomic molecule?

A

A molecule consisting of more than two atoms of the same or different elements

111
Q

Define a covalent bond.

A

The bond that results from the sharing of a pair of electrons by two atoms

112
Q

What is a coordinate covalent bond?

A

A covalent bond in which both of the shared electrons come from the same atom

113
Q

What is bonding capacity?

A

The number of covalent bonds that an atom can form

114
Q

What do Lewis symbols represent?

A

They represent the valence electrons surrounding each of the component atoms as dots

115
Q

What is a Lewis structure?

A

A diagram that shows the valence electrons and the covalent bonds in a molecule

116
Q

What is a structural formula?

A

A representation of the numbers, types, and arrangement of atoms in a molecule, with dashes representing covalent bonds

117
Q

List the states of matter that molecular substances can exist in at SATP.

A

Gases, liquids, and solids

118
Q

What are the typical boiling and melting points of molecular compounds?

A

Relatively low boiling points and melting points

119
Q

Do many molecular substances dissolve readily in water?

A

No, many do not dissolve readily in water

120
Q

What type of forces are intra-molecular forces?

A

Forces of attraction and repulsion within the compound

121
Q

What are inter-molecular forces?

A

Forces of attraction and repulsion between the compound

122
Q

True or False: Covalent bonds are weaker than inter-molecular forces.

A

False

123
Q

What effect does the number of electron pairs in a bond have on bond strength?

A

The strength of the bond increases as the number of electron pairs in the bond increases

124
Q

What is the IUPAC naming system used for?

A

Naming and identifying compounds

The International Union of Pure and Applied Chemistry (IUPAC) provides a systematic approach for naming chemical compounds.

125
Q

Define binary ionic compounds.

A

A compound that consists of ions of only two elements

Examples include NaCl and MgO.

126
Q

Define polyatomic ionic compounds.

A

A compound that consists of ions of more than two different elements

Examples include CaCO3 and HNO3.

127
Q

What is the order of naming in ionic compounds?

A

Metal then non-metal

The non-metal typically has the suffix -ide.

128
Q

What does the criss-cross method refer to in writing chemical formulas?

A

A method to determine the charges of ions and to write the chemical formula

Ensures subscripts are the lowest whole number ratio.

129
Q

What should you do if there is a one in the subscript of a chemical formula?

A

You do NOT have to write it

Subscripts of ‘1’ are typically omitted in chemical formulas.

130
Q

What is a multivalent metal?

A

A metal that can form a variety of cations, each with a different charge

Examples include Fe2+ and Fe3+.

131
Q

How do you indicate the charge of a multivalent cation in a compound’s name?

A

By writing the appropriate Roman numeral in brackets following the name of the ion

Example: Iron (III) oxide.

132
Q

What is the first step in naming ionic compounds with multivalent ions?

A

Recognize that the compound has an element that can have more than one charge

Example: Lead can be +2 or +4.

133
Q

What is the purpose of the reverse criss-cross method?

A

To determine the charge on a multivalent cation

Used after recognizing the multivalent nature of the metal.

134
Q

What is the naming convention for oxyanions with one more oxygen than the ‘–ate’ ion?

A

Add the prefix PER and the suffix -ATE

Example: ClO4- is called perchlorate.

135
Q

What is the naming convention for oxyanions with one less oxygen than the ‘–ate’ ion?

A

Add the suffix -ITE

Example: ClO2- is called chlorite.

136
Q

How do you name a hydrate?

A

Use prefixes to indicate the number of water molecules present

Example: CuSO4 • 5 H2O is named copper(II) sulfate pentahydrate.

137
Q

Fill in the blank: A hydrate is an ionic compound that contains _______ as part of its crystal structure.

A

water

Hydrates include water molecules within their structure.

138
Q

What is the chemical formula for calcium carbonate?

A

CaCO3

Calcium carbonate is a common polyatomic ionic compound.

139
Q

What is the chemical formula for iron(III) hydroxide?

A

Fe(OH)3

Represents an ionic compound with a multivalent metal and a polyatomic ion.

140
Q

True or False: The name of the compound NaCl is sodium chloride.

A

True

Sodium chloride is the standard name for this binary ionic compound.

141
Q

What is electronegativity?

A

The ability of an individual atom, when bonded, to attract the bonding electrons to itself

Developed by Linus Pauling in 1922.

142
Q

Who developed the concept of electronegativity?

A

Linus Pauling

Developed the concept in 1922.

143
Q

Which element has the highest electronegativity?

A

Fluorine

144
Q

Which element has the lowest electronegativity?

A

Francium

145
Q

What does a high electronegativity indicate?

A

An atom is very good at pulling a pair of electrons toward itself.

146
Q

Can electronegativity be measured experimentally?

A

No, it is calculated using physical properties such as ionization energy.

147
Q

What is ΔEN?

A

The difference in electronegativities of two bonded atoms or ions.

148
Q

What does a greater ΔEN indicate about a bond?

A

The more likely it is that the bond is ionic.

149
Q

What type of bond is formed between two identical atoms?

A

Non-Polar Covalent Bond

150
Q

What is the electronegativity difference (ΔEN) in a non-polar covalent bond?

A

ΔEN = 0

151
Q

What characterizes a polar covalent bond?

A

Formed between two atoms with significantly different electronegativities resulting in localized charges.

152
Q

What happens to the electrons in a polar covalent bond?

A

The more electronegative atom pulls the electrons closer, resulting in a partial negative charge.

153
Q

What is the criterion for a bond to be classified as ionic?

A

ΔEN > 1.7

154
Q

What is a polar molecule?

A

A molecule that is slightly positively charged at one end and slightly negatively charged at the other end due to electronegativity differences.

155
Q

What is a key factor that can make a molecule non-polar despite having polar bonds?

A

Symmetry in 3D space.

156
Q

What are the criteria for a compound to be considered polar?

A
  • There are lone pairs of electrons on the central atom
  • It is not symmetrical
  • There is only one atom attached to the central atom
157
Q

What determines the physical properties of a substance?

A

Intermolecular forces.

158
Q

What are Van der Waals Forces?

A

Weak intermolecular attractions that include London Dispersion forces and Dipole-Dipole forces.

159
Q

What causes London Dispersion Forces?

A

A temporary imbalance of electrons within entities.

160
Q

What is a dipole-dipole force?

A

An intermolecular force of attraction between the slightly positive end of one polar molecule and the slightly negative end of an adjacent polar molecule.

161
Q

What is a hydrogen bond?

A

An unusually strong dipole-dipole force between a hydrogen atom attached to a highly electronegative atom (N, O, or F).

162
Q

What role do hydrogen bonds play in DNA?

A

Hold the two helixes of DNA together.

Grade 11 Chemistry (6 decks)

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