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Chem 101 > Topic 2 Flashcards > Flashcards

Topic 2 Flashcards

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1
Q

What are the 3 types of Chemical Bonds?

A

Ionic Bonding
Covalent Bonds
Metallic Bonding

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2
Q

What is Ionic Bonding Between?

A

Metals and Non metals

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3
Q

What is the transfer of electrons in ionic compunds?

A

There is a transfer of electrons to form a Cation and Anion

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4
Q

What is the Physical property of Ionic compounds?

A

They are rigid and brittle

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5
Q

What are Ionic compounds held together by?

A

Electrostatic forces

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6
Q

What is the Conductivity of ionic compounds?

A

They are poor conductors when solid but good conductors when dissolved in water

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7
Q

What are covalent bonds between?

A

2 non-metals

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8
Q

What are the electrons like in Covalent bonds?

A

The non-metals share electrons

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9
Q

What is the structure of Covalent bonds?

A

They have a molecular structure

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10
Q

What States do Molecular structures exist as?

A

They exist as gasses or liquids with low bond polarity

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11
Q

What is the Bond polarity of covalent bonds?

A

Low bond polarity

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12
Q

What are the 2 types of Covalent bonds?

A

Non-polar (Pure Covalent) and Polar

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13
Q

What is the sharing of electrons in Non-polar (pure covalent) bonds?

A

Equal sharing of electrons

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14
Q

Where is equal sharing of electrons found?

A

In diatomic and homonuclear molecules

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15
Q

What is the sharing of electrons in Polar molecules?

A

Unequal sharing of electrons resulting in electronegativity

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16
Q

What does the unequal sharing of electrons cause?

A

Difference in electronegativity

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17
Q

Where is the capacity for an atom to attract electrons found?

A

In a bond

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18
Q

What does a high electronegativity mean?

A

High attractions to electrons

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19
Q

What is the formula to calculate electronegativity?

A

|(First electronegativity)-(Second electronegativity)|

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20
Q

What does an electronegativity of >2 mean?

A

Ionic bond

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21
Q

What does an Electronegativity value of < 2 mean?

A

Polar covalent bond

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22
Q

What does an Electronegativity value of 0 mean?

A

Covalent

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23
Q

What are Metallic Bonds?

A

Bonds between 2 metals

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24
Q

How are electrons in extended structures?

A

A sea of displaced electrons in an extended structures

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25
Q

What are the Physical properties of Metallic bonds?

A

Malleable and ductile and good conductors of heat and electricity.

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26
Q

Which atoms do not obey the octet rule?

A

Atoms in period 3 and beyond

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27
Q

What is the formal charge of an atom?

A

Fc = valence electrons - electrons in lone pairs - 1/2 electrons in covalent bonds

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28
Q

What do lewis structures show?

A

Arrangements of electrons in a molecule but not the molecular shape

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29
Q

What does VSEPR tell us?

A

The molecular shape of atoms

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30
Q

Where does Hybridizing occur?

A

In covalent bonds

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31
Q

What is Hybridizing?

A

The mixing of orbitals to form a new set of orbitals

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32
Q

What is the energy of Hybrid orbitals?

A

The hybrid orbitals are degenerate to each other

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33
Q

What do Single bonds have?

A

Sigma bonds

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34
Q

What do Double bonds have?

A

One sigma and one pi

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35
Q

What do Triple bonds have?

A

2 pi and one sigma

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36
Q

What is Bond Strength related to?

A

It length and energy

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37
Q

How is Bond Strength related to bond length?

A

The greater the bond length the smaller the bond energy

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38
Q

What is Bond Length?

A

The distance that separates nuclei in covalent bonds

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39
Q

Which of bond breaking and forming is exothermic and endothermic?

A

Bond breaking is endothermic and bond forming is exothermic

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40
Q

What is the Formula for Enthalpy of a reaction?

A

(sum of the bond energy of reactants) - (sum of the bond energy of products)

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41
Q

What are Cations and Anions held together by?

A

Electrostatic forces

42
Q

What is the formula for electrostatic forces?

A

q1q2/d^2

43
Q

What is Lattice energy?

A

Lattice energy is the strength of ionic bonds

44
Q

When is Lattice Energy released?

A

When gaseous ions combine to form the ionic solid

45
Q

What is the Atomic Size trend on the period table?

A

It increases as you move down and to the left

46
Q

What does Molecular Orbital theory use as a basis for its ideas?

A

Quantum mechanics

47
Q

Where are electrons found in Molecular Orbital theory?

A

They are found in molecular orbitals

48
Q

What do Molecular Orbitals represent?

A

The delocalization of electrons over an entire molecule

49
Q

What are Molecular Orbitals the result of?

A

The coupling of atomic orbitals

50
Q

What causes Constructive orbitals?

A

Constructive orbitals form when the phase of the atomic orbitals are the same

51
Q

What causes Destructive orbitals?

A

Destructive orbitals form when the phase of the atomic orbitals are different

52
Q

Which are higher energy destructive or constructive molecular orbitals?

A

Destructive molecular orbitals

53
Q

What do sigma bonds form from?

A

Bonds between hybrid orbitals

54
Q

What do pi bonds form from?

A

Bonds between non-hybrid orbitals

55
Q

How are Bond order and Strength related?

A

As bond order increases, bond strength increases

56
Q

What is Bond order a measure of?

A

Bond strength

57
Q

What is electron group configuration based on?

A

The number of electron groups around the central atom

58
Q

What is a Dipole Moment?

A

When a molecule has a slightly positive charge and a slightly negative charge

59
Q

When does Resonance occur?

A

When molecules have more than one plausible lewis structure and the true structure is a resonance hybrid of all the contributing lewis structures

60
Q

What is the formation of molecular orbitals when p atomic orbitals make molecular orbitals?

A

They create 2πp molecular orbitals and 1σbond with the sigma orbital being higher energy than the pi orbital

61
Q

What changes about the molecular orbitals that p forms when it comes to O and F?

A

In O and F the bonding molecular orbitals are flipped so that the 2pi* bonds are higher in energy than the 1σ bond

62
Q

What happens as bond order increases?

A

Bond strength increases so bond length decreases

63
Q

Why are the atomic orbitals of oxygen lower energy than nitrogen?

A

Because oxygen has a higher effective nuclear charge so it holds its electrons more tightly which is more stable

64
Q

How is the energy of orbitals and Zeff related?

A

Orbitals with higher effective nuclear charge hold electrons more tightly so they have a lower energy because they are more stable

65
Q

What is the Arrhenius definition of an Acid?

A

Substance that ionized in a solution to produce H+ or H3O+

66
Q

What is an Arrhenius Base?

A

A substance that ionizes to produce OH- (hydroxide)

67
Q

What is a Bronsted Lowry Acid?

A

A substance that donates H+ to another substance

68
Q

What is a Bronsted Lowry Base?

A

Substance that accepts H+

69
Q

What is a Lewis Acid?

A

An electron-pair acceptor

70
Q

What is a Lewis Base?

A

An electron-pair donor

71
Q

What does complete ionization mean?

A

A strong acid or base

72
Q

What does partial ionization mean?

A

A weak acid or base

73
Q

What makes hybridized orbital bonds?

A

σ bonds

74
Q

What makes unhybridized orbital bonds?

A

π bonds

75
Q

How is the strength of acids and bases measured?

A

By the equilibrium constant, k

76
Q

What is the formula for the equilibrium constant?

A

Products over reactants to the power of their coefficients

77
Q

What does a high acid ionization or base ionization mean?

A

A strong acid or base

78
Q

What does decreasing Ka or Kb mean?

A

Decreasing strength of acid or base

79
Q

What will a strong acid produce?

A

A neutral conjugate base

80
Q

What will a weak acid produce?

A

A weak conjugate base

81
Q

What will a weak base produce?

A

A weak conjugate acid

82
Q

What will a strong base produce?

A

A neutral conjugate

83
Q

What will any compound with a Ka smaller than water produce??

A

A strong conjugate base

84
Q

What are the properties of salt produced in a neutralization reaction?

A

They may or may not produce acid base properties

85
Q

How can you predict the properties of salt produced in a neutralization reaction?

A

By seeing what they come from

86
Q

What does Polyprotic mean?

A

An acid has more than one acidic proton

87
Q

What does Amphoteric or Amphiprotic mean?

A

Something can act as an acid or base

88
Q

What are the types of Weak organic Acids?

A 
Carboxylic acids (ROOH)
Ammonium ions (R3NH+)
89
Q

What are the types of weak organic bases?

A 
Carboxylate ions (RCOO-)
Amines (R3N)
90
Q

What are the Strong acids?

A 
Hydrochloric acid (HCl)
Hydrobromic acid (HBr)
Hydroiodic acid (HI)
Nitric acid (HNO3)
Sulphuric Acid (H2SO4)
Perchloric acid (HClO4)
91
Q

What affects the strength of binary acids?

A

Affected by bond length on bond polarity

92
Q

What is the trend in strength of Binary acids down a group?

A

As you move down a group the acid strength increases?

93
Q

Why does Binary Acid strength increase as you move down a group?

A

Because atom size increases which means bond length increase which means bond strength decreases makes the H+ more easily ionizable

94
Q

What is the Trend of Binary Acid strength as you move across a period?

A

Acid strength increases

95
Q

Why does the Strength of a Binary acid increase as you move across a period?

A

This is because bond polarity increases meaning that the central atom is more electronegative so it attracts electrons more strongly which means the H+ becomes more easily ionizable

96
Q

What factors affect the strength of Oxyacids?

A

The electronegativity of the central atom and the number of oxygens around the central atom

97
Q

What is the trend of oxyacids related to the number of oxygens?

A

As the number of oxygens increases the acid strength increases

98
Q

Why does the acid strength increase as the number of oxygens increase?

A

Because the oxygens are more electronegative so they attract electrons more strongly which makes H+ easily ionizable

99
Q

What is the trend of Oxyacids relating to the central atom?

A

As the electronegativity of the central atom increases the stronger the acid

100
Q

Why does the strength of an acid increase as the strength of the central atom increases?

A

This is because electrons are more tightly held to the negative side which makes the H+ more easily ionizable

Chem 101 (4 decks)

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