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Year 1 Uni > Chemistry Of Drugs > Flashcards

Chemistry Of Drugs Flashcards

1
Q

What is an orbital

A

Region of space around a nucleus that an electron is most likely to occur

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2
Q

Shape of s-orbital

A

Spherical

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3
Q

Highest probability of finding an electron in an s-orbital

A

Nucleus

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4
Q

Shape of p-orbitals

A

Dumbell

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5
Q

Angle of p-orbitals to eachother

A

Orthogonal (right angle)

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6
Q

Probability of finding an electron in a p-orbital at the nucleus and why

A

None
Node at the nucleus

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7
Q

Main reasons atoms bond together

A

Resulting compound is more stable and lower in energy

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8
Q

What does valency mean

A

Number of bonds needed to complete the shell

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9
Q

Valency of carbon and why

A

4
As it has 4 electrons in its outer shell

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10
Q

What is orbital hybridisation

A

Mixing up atomic orbitals to give nee molecular orbitals

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11
Q

Shape and angle of sp3 orbital

A

Tetrahedral
109.5 degrees

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12
Q

Shape and angle of sp2

A

Trigonal planar
120 degrees

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13
Q

Bonds in sp3

A

Sigma
All single

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14
Q

Bonds in sp2

A

One pi bond
Double bond

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15
Q

Shape and angle of sp orbital

A

Linear
180 degrees

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16
Q

Bonds in sp orbital

A

Triple bond

17
Q

What is the strongest covalent bond

A

Sigma

18
Q

How does a sigma bond form

A

Atomic orbitals overlap in a head-on arrangement

19
Q

Formation of a pi bond

A

Overlap of 2 orbital lobes on 1 atom with the orbital lobes on another

20
Q

Where are the electrons in a pi bond

A

Above and below the plane

21
Q

Why are lone pairs held closer to the atom than bonding electrons

A

They exert more repulsion on other valence electrons

22
Q

What is a lone pair

A

A pair of valence electrons not directly involved in bonding

23
Q

Rotation of sigma bonds

A

Free rotation

24
Q

Rotation of pi bonds

A

Fixed oritentation

25
Q

Effect of lone pairs on bond angles

A

Compress then as they repulse the valence electrons

Year 1 Uni (4 decks)

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