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Atomic bonding Flashcards

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1
Q

What are the three types of bonds that atoms can form?

A
  • Ionic bonds
  • Covalent bonds
  • Metallic bonds
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2
Q

What is the valency of Group 1 elements?

A

1

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3
Q

What is the valency of Group 2 elements?

A

2

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4
Q

What is the valency of Group 13 elements?

A

3

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5
Q

What is the valency of Group 14 elements?

A

4

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6
Q

What is the valency of Group 15 elements?

A

3

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7
Q

What is the valency of Group 16 elements?

A

2

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8
Q

What is the valency of Group 17 elements?

A

1

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9
Q

What is an ionic bond?

A

A bond formed by atoms losing and gaining electrons or the attraction between positive and negative ions.

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10
Q

True or False: Transition metals have fixed valencies.

A

False

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11
Q

What is the formula for calcium chloride?

A

CaCl2

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12
Q

What is the formula for aluminium oxide?

A

Al2O3

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13
Q

Fill in the blank: The ionic bond is formed generally between elements of group 1/2/d-block and group ______/______.

A

16, 17

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14
Q

What is the formula for iron(III) sulfate?

A

Fe2(SO4)3

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15
Q

What happens to sodium (Na) when it forms an ionic bond with chlorine (Cl)?

A

Na loses 1 electron and becomes a positive ion (Na+), Cl gains 1 electron and becomes a negative ion (Cl-).

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16
Q

What are the exceptions to the Octet Rule?

A
  • Be shares 2 electrons
  • B and Al share 3 electrons
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17
Q

What is the oxidation state of sulfur in sodium sulfate (Na2SO4)?

A

6

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18
Q

What is the oxidation state of sulfur in sodium sulfite (Na2SO3)?

A

4

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19
Q

What are the three types of bonds that atoms can form?

A
  • Ionic bonds
  • Covalent bonds
  • Metallic bonds
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20
Q

What is the Octet Rule?

A

Atoms gain, lose, or share electrons to have 8 electrons in the outer shell.

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21
Q

Define valency.

A

The number of electrons gained, lost, or shared in a chemical reaction by an atom or group of atoms.

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22
Q

What is a cation?

A

A positive ion that has lost one or more electrons.

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23
Q

What is an anion?

A

A negative ion that has gained one or more electrons.

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24
Q

True or False: Transition metals have fixed valencies.

A

False

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25
What is the formula for calcium chloride?
CaCl2
26
What is the formula for aluminium oxide?
Al2O3
27
Fill in the blank: The ionic bond is formed generally between elements of group 1/2/d-block and group ______/______.
16, 17
28
What is the valency of hydroxide (OH)?
1
29
What is the valency of carbonate (CO3)?
2
30
What is the valency of sulphate (SO4)?
2
31
What is the valency of nitrate (NO3)?
1
32
What is the valency of ammonium (NH4)?
1
33
What is the formula for iron(III) sulfate?
Fe2(SO4)3
34
What happens to sodium (Na) when it forms an ionic bond with chlorine (Cl)?
Na loses 1 electron and becomes a positive ion (Na+), Cl gains 1 electron and becomes a negative ion (Cl-).
35
What are the exceptions to the Octet Rule?
* Be shares 2 electrons * B and Al share 3 electrons
36
What is the oxidation state of sulfur in sodium sulfate (Na2SO4)?
6
37
What is the oxidation state of sulfur in sodium sulfite (Na2SO3)?
4
38
What are the properties of ionic compounds?
High melting point, boiling point, hard, brittle, very soluble in water, conduct electricity when molten or in aqueous solution, react fast.
39
What is a covalent bond?
Bond formed when atoms share electrons.
40
Give an example of a covalent bond formation.
Cl: :Cl + Cl: → Cl2
41
What are the shared electrons in a covalent bond called?
Bonding pairs.
42
What are lone pairs in a covalent bond?
Pairs of electrons in the outer shells that are not involved in bonding.
43
List the properties of covalent substances.
* Low melting point * Low boiling point * Often gases (e.g. oxygen), liquids (e.g. hexane), or soft solids (e.g. butter) * Soluble in non-polar solvents * Solutions do not conduct electricity * React slowly.
44
Fill in the blank: Ionic compounds consist of _______ and _______ throughout, held together by strong ionic bonds.
[positive ions] and [negative ions]
45
True or False: Covalent substances react quickly.
False
46
What type of bond results from the overlap of two s-orbitals?
Sigma bond (σ-bond).
47
What forms a pi bond (π-bond)?
Overlap of two p-orbitals side-to-side.
48
What is the bond energy of a C=C bond?
612 kJ/mol.
49
What happens to ionic compounds in solution?
They react fast because all bonds are broken by the solvent.
50
What are the types of intermolecular forces in covalent substances?
* Dipole-dipole * Hydrogen bonding * Van der Waals forces.
51
How does sugar behave in water?
Soluble in water, but the solution does not conduct electricity.
52
What is a characteristic of polar covalent substances?
They have some ionic properties.
53
What is the result of a double bond?
Consists of a sigma bond and a pi bond.
54
Fill in the blank: Ionic compounds react fast in solution because all bonds are broken by the solvent, so EA = _______.
[0]
55
What is the bond energy of a C-C bond?
348 kJ/mol.
56
What type of reaction do KI and Pb(NO3) undergo?
Fast reaction.
57
What is a Polar Bond?
A bond in which electrons are unequally shared ## Footnote Example: H-Cl, where Cl has a greater attraction for the shared electrons than H.
58
Define Electronegativity.
The relative attraction atoms in a molecule have for the shared electrons.
59
How does electronegativity trend across a period in the periodic table?
Electronegativity increases from left to right due to decrease in atomic radius and increase in nuclear charge.
60
What happens to electronegativity as you move down a group in the periodic table?
Electronegativity decreases due to increase in atomic radius and screening by inner electrons.
61
Who developed the electronegativity scale and what was fluorine's assigned value?
Pauling developed the scale and fluorine was assigned a value of 4.0 (now 3.98).
62
What is the bond energy trend for H-Cl, HBr, and HI?
H-Cl > HBr > HI, because Cl's greater electronegativity results in higher bond energy.
63
What is the significance of placing the more electronegative element last in formulae?
It reflects the order of electronegativity in the bond.
64
What is the difference in electronegativity values that indicates a non-polar covalent bond?
Difference < 0.4.
65
What electronegativity difference indicates a polar covalent bond?
Difference < 1.7.
66
What electronegativity difference indicates an ionic bond?
Difference > 1.7.
67
Define a Polar Molecule (Dipole).
A molecule whose centres of positive and negative charge are separated.
68
Is H-Cl a dipole? Why or why not?
Yes, because H*-Cl- has separated centres of positive and negative charge.
69
Are H2O and NH3 dipoles? Explain.
Yes, their non-symmetrical shape gives them separate centres of positive and negative charge.
70
Are CO and CO2 dipoles? Why or why not?
No, because their symmetrical shape cancels out the polarity of their bonds.
71
What determines the dipole moment?
The size of the positive/negative charge (q) and the distance (d) of separation.
72
What evidence supports the non-linear shape of water?
Water has a dipole moment, while carbon dioxide does not.
73
What is the shape of all diatomic molecules?
Linear ## Footnote Example: H2
74
What does the Electron Pair Repulsion Theory (VSEPR) predict about the shape of molecules?
Electron pairs around the central atom repel each other.
75
What is the bond angle and shape when there are 2 electron pairs?
180°, linear.
76
What is the bond angle and shape when there are 3 electron pairs?
120°, planar trigonal.
77
What is the bond angle and shape when there are 4 electron pairs?
109.5°, tetrahedral.
78
How do lone pairs affect bond angles in molecular shapes?
Lone pairs repel more than bonding pairs.
79
What is the bond angle and shape for 4 pairs with 1 lone pair?
Bond angle < 109°, pyramidal.
80
What is the bond angle and shape for 4 pairs with 2 lone pairs?
Bond angle << 109°, planar V-shape.
81
What is the shape of a molecule with 2 double bonds?
Linear ## Footnote Example: O=C=O
82
What is the shape of PCl5?
Trigonal bipyramidal.
83
What is the shape of a molecule with 1 double bond and 1 triple bond?
Linear ## Footnote Example: H-C≡N
84
What is the shape of a molecule with 1 double bond and 2 single bonds?
Planar trigonal ## Footnote Example: H2C=O
85
What are the hybrid orbitals used to explain molecular shapes?
sp, sp², sp³, sp³d, sp³d².
86
What shape is associated with sp hybridization?
Linear.
87
What shape is associated with sp² hybridization?
Planar trigonal.
88
What shape is associated with sp³ hybridization?
Tetrahedral.
89
What shape is associated with sp³d hybridization?
Trigonal bipyramidal.
90
What shape is associated with sp³d² hybridization?
Octahedral.
91
What are van der Waal's forces?
Forces between non-polar molecules. Very weak forces.
92
Give examples of non-polar substances that exhibit van der Waal's forces.
* H2 (g) * O2 (g) * CH4 (g) * Cl2 (g) * Br2 (l) * I2 (s) * C2H6 (l)
93
What is the relationship between the number of electrons in a molecule and van der Waal's forces?
The more electrons in the molecule, the bigger the forces.
94
What effect do van der Waal's forces have on the state of non-polar substances?
They allow liquefaction of gases like H2 and O2.
95
What is dipole-dipole attraction?
Forces between polar molecules.
96
What is hydrogen bonding?
Forces between molecules which have hydrogen bonded to a highly electronegative element such as F, O, N, or Cl.
97
List some effects of hydrogen bonding.
* Water has a high melting and boiling point. * Water dissolves other polar and ionic compounds. * Ice is less dense than water. * Ethanol and ammonia dissolve in water.
98
True or False: Water dissolves non-polar substances like iodine and oxygen.
False.
99
What is ion-dipole attraction?
Forces between ions and polar molecules.
100
What is ion-ion attraction?
Ionic bond. Very strong bonds.
101
What is the process for a solution to occur?
Solution forces (A-B) must overcome solute and solvent forces.
102
What does 'like dissolves like' mean?
Polar solutes dissolve in polar solvents, and non-polar solutes dissolve in non-polar solvents.
103
Fill in the blank: Polar solutes do not dissolve in _______ solvents.
non-polar
104
What is the lattice energy of NaCl?
770 kJ mol-1.
105
At what temperature does water have maximum density?
4°C.
106
What happens to the structure of water at 0°C?
A 4th hydrogen bond is formed, directed to the 4th corner of a tetrahedron.
107
What is solubility product (S.P.)?
The equilibrium constant expression is the product of the ions.
108
What is the relationship between ionization and solubility for NH3 and HCl?
Ionization increases the solubility of NH3 and HCl.
109
True or False: Weak van der Waals forces in solution can overcome strong dipole-dipole/hydrogen bonding.
False.
110
What is the significance of entropy (S) in the formation of solutions?
Entropy must be considered, and the requirement for solution is AG = -.
111
What does a large positive AS indicate in terms of solubility?
It can cause an endothermic solution.
112
What is the general rule for good river water regarding dissolved oxygen?
Good river water has ~ 10 mg dm-3 (ppm) dissolved oxygen.
113
What are the two types of solids?
Amorphous and Crystalline
114
What is the pattern of particle arrangement in crystals called?
Lattice
115
Name three types of lattices.
* Cubic * Face-centred cubic * Hexagonal close packed
116
What do we call substances that have more than one lattice arrangement?
Polymorphic
117
Give an example of a polymorphic substance.
NaCl (cubic, octahedral), Carbon (diamond, graphite)
118
What are allotropes?
Different physical forms of an element
119
What type of crystal is NaCl?
Ionic crystal
120
What are the units occupying the lattice points in ionic crystals?
+ and - Ions
121
What type of bonds do ionic crystals primarily have?
Ionic bonds
122
List the types of binding forces in molecular crystals.
* van der Waals forces * Hydrogen bonding * Dipole-dipole interactions
123
What is the structure of metallic bonds?
+ ions in a 'sea' of valence electrons
124
What are the properties of ionic crystals?
* High melting point * High boiling point * Hard * Brittle * Insulators * Soluble in water (polar solvents)
125
What are the properties of molecular crystals?
* Low melting point * Low boiling point * Very soft * Insulators * Soluble in non-polar solvents (like hexane) * Soluble in water (polar solvent)
126
What are the properties of covalent crystals?
* High melting point * High boiling point * Insulators (except graphite) * Insoluble
127
What is diamond classified as?
Covalent crystal
128
How are atoms arranged in diamond?
Tetrahedrally arranged, held by strong covalent bonds
129
What makes diamond very hard?
Strong covalent bonds
130
What is the structure of graphite?
Carbon atoms covalently bonded to 3 other carbons, forming layers
131
How does graphite conduct electricity?
The fourth electron in each carbon atom forms a continuous bond that allows electron movement across layers
132
What holds the layers of graphite together?
Very weak van der Waals forces
133
What are the two important allotropes of iron?
* Austenite (fcc) * Ferrite (bcc)
134
What happens during tempering of steel?
Heating steel to various temperatures below 723°C and then cooling it to remove carbon
135
What is quenched steel known for?
Being hard and unmalleable
136
Fill in the blank: In ice, a fourth hydrogen bond is formed, directed to the _______.
fourth corner of a tetrahedron
137
True or False: All allotropes are crystalline.
False

Chem Chem (2 decks)

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