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BIO1332 - Biochemistry > Chemical Bonding > Flashcards

Chemical Bonding Flashcards

1
Q

What group is the Nobel gases in?

A

Group 8

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2
Q

What are the 6 Nobel gases?

A
  • He
  • Ne
  • Ar
  • Kr
  • Xe
  • Rn
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3
Q

How many electrons do Nobel gases have in there outer electron?

A

8

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4
Q

Describe novel gases:

A
  • Very stable and un-reactive or inert
  • Monatomic
  • Dont normally form bonds with other elements
  • Do not need to gain, lose or share electrons
  • Lewis Octet rule
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5
Q

What does monatomic mean?

A

They exist as individual atoms

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6
Q

What are valance shells?

A
  • Outermost occupied shell of an atom
  • Highest principle quantum number
  • Most likely to participate in bonding
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7
Q

What will atoms without 8 electrons in the valence shells will form?

A

Chemical bonds with other atoms

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8
Q

What are chemical bonds made from?

A

Electrons

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9
Q

How do atoms make bonds?

A

Atoms must collide with each other to make bonds

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10
Q

What are the two types of electrons in an atom?

A
  • Core electrons

- Valance electrons

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11
Q

Define ionic bonds:

A

Is the electrostatic attraction that forms between oppositely charged ions

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12
Q

What two main ways for atoms bond with other bonds?

A
  • Ionic bonding

- Covalent bonding

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13
Q

Define covalent bond:

A

is a shared pair of electrons between atoms

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14
Q

What happens between atoms in ionic bonding?

A
  • Atoms gain or loss electrons to fulfil the octet rule

- Atoms become ions

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15
Q

Atoms that lose electrons have more or less proton than electrons?

A

More

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16
Q

Atoms that gain electrons have more or less protons to electrons?

A

Less

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17
Q

Do atoms become positively or negatively charged when they lose electrons?

A

Positive

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18
Q

Do atoms become positively or negatively charged when they gain electrons?

A

Negative

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19
Q

What are atoms called when they lose electrons?

A

cations

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20
Q

What elements normally lose electrons?

A

S and d block elements

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21
Q

What aerators called when they gain electrons?

A

Anions

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22
Q

What elements normally gain electrons?

A

P block elements

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23
Q

What charge do ionic compounds have?

A

Neutral charge

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24
Q

If ionic compounds have a neutral charge what must the total of cations equal to the total of anions?

A

Cations and anions must be equal

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25
Q

What are ionic lattices?

A

Ionic compounds form giant 3D structures

26
Q

What are diatomic?

A

Two atoms joined tother by a covalent bond

27
Q

Give an example of diatomics:

A

Fluorine
Chlorine
Oxygen
Nitrogen

28
Q

Describe Fluorine:

A
  • 9F so 1s2, 2s2, 2p5
  • F atom requires 1 electron for full valence shell
  • Forms diatomic fluorine molecule, F2
  • Single F-F bond
29
Q

Describe chlorine:

A
  • 17Cl so 1s2, 2s2, 2p6, 3s2, 3p5
  • Cl atom requires 1 electron for full valence shell
  • Forms diatomic chlorine molecule,Cl2
  • Single Cl-Cl bond
30
Q

Describe oxygen:

A
  • 8O so 1s2, 2s2, 2p4
  • O atom requires 2 electrons for full valence shell
  • Forms diatomic oxygen molecule, O2
  • Double O=O bond
31
Q

Describe nitrogen:

A
  • 7O so 1s2, 2s2, 2p3
  • N atom requires 3 electrons for full valence shell
  • Forms diatomic oxygen molecule, N2
  • Triple N≡N bond
32
Q

How can covalent bonds be represented by?

A

By lines or wedges

33
Q

What determines whether the bond is ionic or covalent?

A

Electronegativity

34
Q

What is electronegativity?

A

Ability of an atom to pull electrons towards itself

35
Q

Finish the sentence:

An atom with a high electronegativity pulls electrons…

A

more strongly towards itself

36
Q

In which direction does does electronegativity increase on the period table?

A
  • horizontally left to right

- vertically down to up

37
Q

What is the Pauling scale of electronegativity?

A

Increase electronegativity across the periodic table

38
Q

What does electronegativity depend on?

A
  • Nuclear charge
  • Atomic radius
  • Electron shielding
39
Q

What does an atom need to have high electronegativity?

A
  • Higher nuclear charge
  • Small atomic radius
  • Low amount of shielding
40
Q

If the difference in values of electronegativity is greater than 1.7 is it more likely to form covalent or ionic bonds?

A

Ionic bonds

41
Q

If the difference in values of electronegativity is less than 1.7 is it more likely to form covalent or ionic bonds?

A

Covalent bonds

42
Q

If the difference in values of electronegativity is equal to 1.7 what bond is it more likely to form?

A

Polar covalent bond

43
Q

Why is hydrogen chloride a special case?

A
  • Gaseous form are polar covalently bonded
  • Aqueous form ionises completely to give cation and anions
  • Electronegativity difference is 0.9
44
Q

What electronegativity differences do covalent bonds have?

A

0.0

45
Q

What electronegativity differences does polar covalent bonds have?

A

0.9

46
Q

What electronegativity differences does ionic bonds have?

A

2.1

47
Q

What differences do compounds with ionic bonds have compared to covalent bonds?

A
  • Boiling point
  • Melting point
  • Solubility in water
  • Electrical conductivity
48
Q

What charge does phosphate ion have?

A

-3

49
Q

What charge does sulphate ion have?

A

-2

50
Q

What charge does carbonate ion have?

A

-2

51
Q

What charge does nitrate ion have?

A

-1

52
Q

What charge does hydroxide ion have?

A

-1

53
Q

What charge does ammonium have?

A

+1

54
Q

Is hydrogen sulphate an acid or base?

A

Acid

55
Q

Is hydrogen nitrate an acid or base?

A

Hydrogen nitrate

56
Q

Is sodium carbonate an acid or base?

A

base

57
Q

Is sodium hydroxide an acid or base?

A

base

58
Q

Do all electrons in covalent bonds need to bonded?

A

No

59
Q

What are lone pairs?

A

Unbonded pairs of electrons

60
Q

What are dative covalent bonds?

A

Lone pairs can be shared with ions

BIO1332 - Biochemistry (19 decks)

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