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Biochemistry :) > Organic Chem: Intro > Flashcards

Organic Chem: Intro Flashcards

1
Q

Which group of the periodic table is carbon in?

A

14

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2
Q

How many valence electrons does carbon have?

A

4

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3
Q

What is carbon’s electron configuration?

A

1s^2 2s^2 2p^2

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4
Q

What is carbon’s valence shell configuration?

A

2s^2 2p^2

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5
Q

What is carbon’s electronegativity?

A

2.5

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6
Q

What is electronegativity?

A

How much an atom attracts a bonding pair of electrons

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7
Q

What bond type is expected for carbon?

A

Covalent: between atoms with equal electronegativity

Polar covalent: between atoms with differing electronegativity

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8
Q

What is an empirical formula?

A

The simplest whole number ratio of elements

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9
Q

What is carbon’s empirical formula?

A

C3H7

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10
Q

What is a molecular formula?

A

The actual number of atoms of each element

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11
Q

What is carbon’s molecular formula?

A

C6H14

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12
Q

What is a structural formula?

A

Minimal detail for an unambiguous structure

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13
Q

What is a displayed formula?

A

Relative placing of atoms and bonds between them

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14
Q

What is a skeletal formula?

A

The carbon skeleton and functional groups only

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15
Q

What is a sigma bond?

A

End to end overlap bond
Orbitals overlap as two atoms approach
Electrons of one atom attracted to nucleus of the other
This continues until repulsion between nuclei outweighs this attraction

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16
Q

Describe the structure of methane.

A

Four C-H bonds of identical length and tetrahedral geometry

Bond angle: 109.5 degrees

17
Q

How do we know s and p orbitals get mixed to form hybrid orbitals?

A

A carbon atom in ground state wouldn’t form four single bonds
Promoting a 2s electron into an empty 2p orbital gives 4 unpaired electrons
Methane would have 4 bonds in this case, but one would be a different length
However, all four bonds in methane are equal
So, the bonding atomic orbitals of carbon must be equivalent
s and p orbitals get mixed to form hybrid orbitals

18
Q

What is sp^3 hybridisation?

A

One s and three p orbitals getting mixed

19
Q

Describe sp^2 hybridisation.

A

One s and two p orbitals mix
Gives bond angle of 121.3 degrees
When carbon is only bonding to three atoms
The three hybrid orbitals can form three sigma bonds

20
Q

What can form a pi bond in sp^2 hybridisation (e.g. ethene)?

A

The two pure p orbitals of the two carbon atoms can overlap sideways to form a pi bond

21
Q

Describe the structure of benzene.

A

Planar molecule
Each carbon atom is sp^2 hybridised
6 electrons in pure p orbitals capable of overlapping
Get delocalisation over the ring

22
Q

What is sp hybridisation?

A

Mixing one s orbital and one p orbital to obtain two sp hybrid orbitals

23
Q

How many pure p orbitals are left over per carbon atom in sp hybridisation and what does this mean?

A

Two pure p orbitals are left over per C so two pi bonds are formed
Each carbon atom forms two sigma bonds and two pi bonds

24
Q

What are some properties of organic compounds?

A

Physical and chemical behaviour of organic compounds are heavily influenced by the polarity of the molecule
Most organic compounds are not soluble with water
Organic compounds with oxygen and nitrogen atoms are somewhat soluble because the electronegative atoms form hydrogen bonds with water
Many organic compounds undergo combustion and burn vigorously in air

25
Q

Why is a covalent bond between two carbon atoms non-polar?

A

Because the electrons are shared equally

26
Q

Are most elements found in organic compounds more or less electronegative than carbon?

A

More electronegative than carbon (except hydrogen which has electronegativity value of 2.1)

27
Q

What is the polarity of a molecule determined by?

A

The polarity of its bonds and the structure of the molecule

28
Q

What are the two major classes of organic compounds?

A

Aromatic

Aliphatic

29
Q

What is an aromatic organic compound?

A

Contain cyclic conjugated double bond system with 4n + 2 pi electrons

30
Q

What is an aliphatic organic compound?

A

All other compounds without such ring system

31
Q

What are functional groups?

A

Characteristic structural features

32
Q

Define oxidation.

A

When carbon atoms are oxidised they often form additional bonds to oxygen

33
Q

Define reduction.

A

When carbon atoms are reduced they often form additional bonds to hydrogen

34
Q

Define substitution.

A

Exchange of one atom in a molecule with another atom or group of atoms

35
Q

Define elimination.

A

A single reactant is split into two products

36
Q

Define addition.

A

Two reactants add together to form a single product

Biochemistry :) (9 decks)

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