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Chemistry > Bonding > Flashcards

Bonding Flashcards

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1
Q

What are the 3 types of chemical bond?

A
  • Ionic
  • Covalent (polar/non-polar)
  • Metallic
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2
Q

What does an ionic bond form between?

A

A metal and a non-metal

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3
Q

If an electron is lost, what charge does the particle have?

A

Positive

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4
Q

If an electron is gained, what charge does the particle have?

A

Negative

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5
Q

What is a positively charged ion called?

A

Cation

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6
Q

What is a negatively charged ion called?

A

Anion

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7
Q

What is a covalent bond?

A

A bond formed between atoms by the sharing of electrons

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8
Q

What is a non-polar covalent bond?

A

When electrons are shared equally

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9
Q

What is a polar covalent bond?

A

When electrons are shared unequally

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10
Q

What is the electron domain geometry of minimum repulsion?

A

Tetrahedral

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11
Q

What is the trend in electronegativity in the periodic table?

A

Increased from left to right (across periods)

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12
Q

What model is based on the idea that electron pairs will repel each other?

A

Valence shell electron pair model (VSEPR)

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13
Q

How many electron domains are there?

A

4

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14
Q

What are electron domains?

A

Where electrons are likely to be found

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15
Q

What is the electron domain geometry of water?

A

Tetrahedral

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16
Q

What is the molecular geometry of water?

A

Bent

17
Q

What is the electron domain geometry for carbon dioxide?

A

Linear shape

18
Q

What is the electron domain geometry for boron trifluoride (BF3)?

A

Trigonal planar

19
Q

What is the electron domain geometry for methane?

A

Tetrahedral

20
Q

What is lattice energy?

A

A measure of the stabilisation caused by oppositely charged ions forming a solid lattice

21
Q

What do polar covalent bonds result in?

A

A dipole

22
Q

What is electronegativity?

A

The ability of an atom in a molecule to attract electrons to itself

23
Q

Why is electronegativity so important?

A

Intermolecular electrostatic interactions means water is liquid at room temperature

24
Q

What is valence bond theory

A
  • When a valence atomic orbital of one atom merges with that of another atom
  • Orbitals overlap
25
Q

What does Lewis theory state?

A

That covalent bonding occurs when atoms share electrons, which concentrates the electron density between the nuclei

26
Q

What are sigma bonds?

A

Covalent bonds in which the electron density is concentrated symmetrically about the internuclear axis

27
Q

What are pi bonds?

A

Bonds that form as a result of sideways overlap of 2p orbitals, in which the overlap regions lie above and below the internuclear axis

28
Q

Describe a sp hybrid orbital

A
  • 2 lobes
  • One is lever than the other
  • Identical in shape
  • Opposite direction
29
Q

Which bond has lower energy levels; sigma or pi?

A

Sigma

30
Q

Why do orbitals hybridise?

A
  • The large lobe of hybrid orbitals can be better directed at other atoms than unhybridised atomic orbitals
  • They overlap more strongly, resulting in stronger bonds
31
Q

What is the uncertainty principle?

A

Impossible to say where an electron is at any given time

32
Q

What is a lone pair?

A

A pair of electrons in a fully occupied orbital

33
Q

Where do covalent bonds form?

A

Between 2 non metals

Chemistry (8 decks)

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