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Chemistry Unit 1 > Structure And Bonding > Flashcards

Structure And Bonding Flashcards

1
Q

Describe pure covalent bonding

A

The shared pair of electrons is shared equally by the atoms in the molecule

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2
Q

Describe polar covalent bonding

A

Unequal sharing of the bonded electrons. Which causes one atom to have a slightly negative charge, and the other having a slightly positive charge

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3
Q

What do polar covalent bonds create?

A

Permanent dipoles

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4
Q

Explain electronegativity

A

A numerical measurement on a scale of 0-4 (low to high) used to sssess an elements ability to attract bonded electrons

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5
Q

What does the difference in electronegativity between atoms in a compound show?

A

An indication of the type of bonding present

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6
Q

Describe the bonding continuum

A

The type of bonding changes gradually as the difference in electronegativity between atoms increases

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7
Q

What is at either ends of the bonding continuum?

A

Ionic bonding at one end and pure covalent bonding at the other

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8
Q

What is in the middle of the bonding continuum?

A

Polar covalent bonding

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9
Q

What are intermolecular forces, and what is the other name they are known by?

A

Act between molecules, known as van der waals forces

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10
Q

Name the three types of van der waals forces

A

London dispersion forces
Permanent dipole- permanent dipole interactions
Hydrogen bonding

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11
Q

Describe London dispersion forces

A

Weak attractions between temporary dipoles in molecules, and are significant between non-polar molecules

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12
Q

Describe permanent dipole-permanent dipole interactions.

A

Attractions between polar molecules which have permanent dipoles

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13
Q

When will a molecule only be polar?

A

If one side of the molecule is slightly positive and the other is slightly negative

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14
Q

When do hydrogen bonds form?

A

Form between highly polar molecules which have hydrogen bonded to the greatly electronegative elements

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15
Q

What’s are the highly electronegative elements that allow for hydrogen bonds when they are bonded with hydrogen?

A

Fluorine
Oxygen
Nitrogen

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16
Q

What does hydrogen bonds give compounds that is unusual?

A

Unusually high melting and boiling points

17
Q

Why do hydrogen bonding give unusually high melting and boiling points?

A

Because they are the strongest van der waals forces so they need more energy to separate the molecules

18
Q

An example of hydrogen bonding?

A

Water

19
Q

When water is cooled to 4 degreees Celsius what happens?

A

It expands and decreases density

20
Q

Why does water expand and decrease density when cooled?

A

The water molecules form a more open structure with increased hydrogen bonding

21
Q

Compounds with molecules and which have hydrogen bonds between them are more viscous than?

A

Compounds with molecules which have other intermolecular forces

22
Q

The polar nature of water makes it a good solvent for what type of compounds?

A

Ionic and polar covalent compounds

23
Q

Non-polar solvents can dissolve what type of substances?

A

Non-polar substances

24
Q

The molecules of polar covalent liquids which are miscible with water form hydrogen bonds with?

A

Water molecules

25
Q

What do polar covalent bonds create?

A

Permanent dipoles

26
Q

What does the difference in electronegativity between atoms in a compound show?

A

An indication of the type of bonding present

27
Q

What are intermolecular forces, and what is the other name they are known by?

A

Act between molecules, known as van der waals forces

28
Q

When will a molecule only be polar?

A

If one side of the molecule is slightly positive and the other is slightly negative

29
Q

What’s are the highly electronegative elements that allow for hydrogen bonds when they are bonded with hydrogen?

A

Fluorine
Oxygen
Nitrogen

30
Q

What does hydrogen bonds give compounds that is unusual?

A

Unusually high melting and boiling points

31
Q

Why do hydrogen bonding give unusually high melting and boiling points?

A

Because they are the strongest van der waals forces so they need more energy to separate the molecules

32
Q

Why does water expand and decrease density when cooled?

A

The water molecules form a more open structure with increased hydrogen bonding

33
Q

Compounds with molecules and which have hydrogen bonds between them are more viscous than?

A

Compounds with molecules which have other intermolecular forces

34
Q

Is water polar or non-polar?

A

Polar

35
Q

The polar nature of water makes it a good solvent for what type of compounds?

A

Ionic and polar covalent compounds

36
Q

Non-polar solvents can dissolve what type of substances?

A

Non-polar substances

37
Q

The molecules of polar covalent liquids which are miscible with water form hydrogen bonds with?

A

Water molecules

Chemistry Unit 1 (3 decks)

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