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Chemistry > Chemical Bonding Unit 1 > Flashcards

Chemical Bonding Unit 1 Flashcards

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1
Q

7 main VSEPR types

A

Linear
Trigonal Planar
Tetrahedral
Triangular Pyramidal
Angular/Bent
Triangular Bi-Pyramidal
Octahedral

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2
Q

Type and class

A

AX2
Linear

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3
Q

Type and class

A

AX3
Trigonal Planar

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4
Q

Type and class

A

AX4
Tetrahedral

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5
Q

Type and class

A

AX3E
Triangular Pyramidal

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6
Q

Type and class

A

AX2E2
Angular/Bent

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7
Q

Type and class

A

AX2E
Bent

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8
Q

Type and class

A

AXE3
Linear

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9
Q

Type and class

A

AX6
Octahedral

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10
Q

Type and class

A

AX5
Triangular Bi-Pyramidal

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11
Q

Why do chemical bonds form?

A

To fill valence shell

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12
Q

How many ways can an atom obtain a full valence, shell, and how?

A

They can either gain or lose electrons, which is known as ionic bonding

They can share electrons between atoms. This is covalent bonding.

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13
Q

How do you determine if an atom shares electrons or transfers electrons

A

Through electronegativity, it’s a number that decides the desire, and Atom has for a pair of electrons

The larger the number the more Adam wants electrons

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14
Q

How do you determine if a bond is ionic or covalent?

A

By looking at the difference between their electronegativities

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15
Q

Electronegative chart

A
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16
Q

When do ionic bonds form?

A

When electrons are transferred from one atom to another

17
Q

What is the strongest bond possible?

A

Ionic bonds

18
Q

What do ionic compounds form and not form?

A

They form crystals otherwise known as a crystal lattice

They don’t form molecules

19
Q

How are covalent bonds formed?

A

They’re formed when electrons are shared between atoms

20
Q

Ways for atoms to share electrons

A

When shared equally the bond is nonpolar

When shared unequally, the bond is polar

21
Q

How do you know which side of a bond is slightly negative and which side is slightly positive?

A

The atom that has the most electrons will become slightly negative

22
Q

How to draw E-dot diagrams

A

Use the octet rule where atoms want eight valence electrons

23
Q

Four steps in drawing an E-dot diagram

A

1.) how many atoms of each element are in the molecule

2.) figure out which atoms are connected.

3.) determine the number of dots

4.) decide where the dots go.

24
Q

What is a double bond?

A

When two pairs of electrons are shared

25
Q

Seven. Exceptions to the octet rule.

A

1.)H only needs two valence electrons.

2.) alkaline metals only need 2

3.) B and down only need six.

4.) Be only needs four.

5.) phosphorus can have up to 10 valence electrons.

6.) sulphur can have up to 12.

7.) sometimes tin will only need six.

26
Q

What is a resonance structure?

A

A structure used when no single structure adequately represents the molecule 

27
Q

VSEPR and what it means

A

Valence shell electron pair repulsion theory

Pairs of electrons repel each other, in order to get as far apart as possible

28
Q

What is intermolecular attraction?

A

Attraction between different molecules

Ex:

29
Q

What is intra-molecular attraction?

A

Attraction within the same molecule

30
Q

What is a dipole?

A

When one end of the molecule is slightly positive and the other end of the molecule is slightly negative

31
Q

What happens when a molecule has a slightly positive, charged a slightly negatively charged end

A

The molecule have a dipole-dipole attraction

32
Q

Which has a higher attraction and why

A

Left

The bond is between hydrogen and oxygen

33
Q

What is an H bond?

A

An attraction between hydrogen from one molecule, and a molecule of nitrogen, oxygen, or fluorine from another

34
Q

How much stronger are hydrogen bonds than dipole dipole?

A

10 times stronger

35
Q

What are London forces?

A

The result of an unequal distribution of electrons in a molecule

36
Q

Where are London forces present?

A

In all molecules, but significant in nonpolar

37
Q

Types of intermolecular forces, and what they are known as

A

1.) H-bonds
2.) dipole-dipole
3.) London forces

Known as Vander waals forces

38
Q

Does H2O or H2S have a higher boiling point and why

A

H2O because it has a hydrogen bond (NOF)

Chemistry (6 decks)

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