eLFH - Chemical Bonds and Reactions Flashcards

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1
Q

Why do bonds occur

A

Atoms tend to their lowest energy by giving, receiving or sharing electrons to get filled and stable orbitals when possible

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2
Q

Forms of bonds created by electrons holding atoms in association

A

Sharing electrons - covalent bonds

Transferring electrons - ionic bonds

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3
Q

Covalent bonds definition

A

Shared electrons in outer orbitals form strong covalent bonds

E.g. Carbon has 4 electrons in outer orbital with maximum possible 8
Hydrogen has 1 electron in outer orbital with maximum possible 2
Therefore CH4 forms with covalent bonds to fully occupy all outer orbitals

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4
Q

Ionic bonds definition

A

Transfer of electron from one outer orbital to another
Electrostatic forces then hold atoms together

E.g. Chloride atom will attract the single electron from outer orbital of Sodium thus giving both stable outer orbitals
Leaves Cl- and Na+ charges and ionic attraction keeps atoms together

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5
Q

Which bond is stronger - covalent or ionic

A

Covalent bonds are stronger

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6
Q

What happens to strength of bond and shape of molecule as number of shared electrons increases

A

Strength of bond increases with increased number of shared electrons

Free rotation also decreases and therefore molecules become more rigid, and isomerism results

Atoms in molecules bond in different ways depending on conditions in which they are joined, and exert differing properties

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7
Q

Types of forces that give molecules specific 3D shapes

A

Hydrogen bonding
Hydrophobic bonding
Van der Waals forces

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8
Q

Hydrogen bond definition

A

Hydrogen atom covalently bound to another atom
Hydrogen atom becomes positive and other atom negative charged

Creates dipolar attractive force

Therefore positive hydrogen atom in molecule attracts to negatively charged atom on another of the same molecule within the substance

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9
Q

Hydrophobic bond definition

A

Non polar molecules interact to exclude water molecules from between them
E.g. phospholipid bilayer

Molecules behave in this way to achieve lower energy state

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10
Q

Van der Waals forces definition

A

Weak intermolecular forces of attraction between electron clouds of neighbouring atoms

Weak but numerous so become more important

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11
Q

Types of repulsive forces that act on molecules to prevent aggregation

A

Electrostatic repulsion

Steric hindrance

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12
Q

Electrostatic repulsion definition and example

A

Similarly charged molecules with repel

E.g. RBCs have net negative electrical charge, therefore do not aggregate

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13
Q

Steric hindrance definition

A

Certain parts of molecules will be larger or smaller than others, and may have rigid shapes

Therefore certain molecule combinations will be impossible
E.g. jigsaw pieces that don’t fit

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14
Q

Organic chemistry definition

A

Study of carbon molecules

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15
Q

Examples of groups that can be attached to chains of carbon molecules

A

Hydroxyl

Amino

Carboxyl

Methoxy

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16
Q

Hydroxyl group

A

OH

17
Q

Amino group

A

NH2

18
Q

Carboxyl group

A

COOH2

19
Q

Methoxy group

A

OCH3

20
Q

Aromatic compounds

A

Typified by benzene ring

Six carbons joined to form a ring

21
Q

Phenol group

A

Benzene ring with a hydroxyl group

22
Q

Propofol chemical make up

A

Benzene ring with hydroxyl group (phenol)
With 2 carbon chains attached

23
Q

Propofol chemical name

A

2, 6 Di-isopropylphenol