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Semester 1 Revision > Chemistry Clinical Sciences 4-6 > Flashcards

Chemistry Clinical Sciences 4-6 Flashcards

1
Q

Mass, Moles and Mr Equation

A

Moles= Mass/ Mr

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2
Q

How many molecules in 1 mole?

A

23

6.02 x 10

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3
Q

What is a mole?

A

A mole is the same as Avogadro’s number which is the number of Atoms found in 12g of Carbon-12.

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4
Q

What is molar mass?

A

The mass of 1 mole of the substance.

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5
Q

If you have the moles of a substance:

a) how would you find the number of molecules?
b) how would you find the mass of a substance?

A

a) Multiply by the Avogadro’s Constant.

b) Multiply by the Molar Mass

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6
Q

What volume does 1 mole of ANY gas occupy?

A

Occupies the same VOLUME at standard pressure and temperature.

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7
Q

What is the Gas Equation and what does each letter stand for?

A 
PV= NRT
P= Pressure is 100kPa
R is a constant 
T= Temperature is 273K
V= Volume is 22.4 L
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8
Q

How do you work out the concentration of solutions?

A

Molarity (mol/L)= Number of Moles/ Volume in Litres.

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9
Q

What is Molarity?

A

The SOLUTION CONCENTRATION expressed as number of moles of solute dissolved in 1 litre of solution.

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10
Q

What equation represents the Concentration of Solutions?

A

C1 x V1 = C2 x V2

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11
Q

Conversions:

mg to G + G to mg

A

x1000

/1000

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12
Q

Conversions:

ml to L + L to ml

A

x1000

/1000

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13
Q

Conversions:
Microlitres to Litres
Litres to Microlitres

A

x1,000,000

/1,000,000

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14
Q

Conversions:
Nanolitres to Litres
Litres to Nanolitres

A

x1,000,000,000

/1,000,000,000

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15
Q

What do Chemical Reactions involve?

A

Compound changing identity
Energy changes
Breaking/ Making of bonds
Rearrangement of valent electrons

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16
Q

What do Chemical Equations describe?

A

Symbols represent elements
Formula describe composition of compounds
Show changes in compounds

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17
Q

What is the percentage yield equation?

A

Percentage Yield= Actual Yield/ Theoretical Yield (x100).

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18
Q

What does Quantum theory explain?

A

Explains the nature and behaviour of matter and explains energy on a atomic and subatomic level.

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19
Q

What 3 observations can Quantum theory explain which classical mechanics cannot?

A

Spectra of light emitted by atoms- How much light is given out by atoms.
Electrons in an atom are stable and stay in their orbitals.
Light can behave as if it is made up of photons with energy depending on frequency.

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20
Q

What is the uncertainty principal?

A

You will never know both the exact location and velocity of a subatomic particle at the same time.

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21
Q

How are electrons described by the Schrodinger equation? How are electrons written in the Schrodinger equation?

A

As waves but are written as quantum numbers.

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22
Q

When an electron absorbs a photon of light, what does this allow the electron todo?

A

In atoms electrons are in energy levels. ABSORPTION of a PHOTON of light allows an electron to JUMP UP to a HIGHER level.

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23
Q

What does measuring the energy of the photon show us?

A

The energy difference between levels to be determined which showed ENERGY LEVELS are NOT EQUALLY spaced.

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24
Q

What is ionisation energy?

A

An ionisation energy is the AMOUNT of ENERGY needed to REMOVE ELECTRONS from atoms/ ions.

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25
Q

What is the DEFINITION of first ionisation energy?

A

DEFINTION: First ionization energy is the energy required to remove one mole of electrons (to infinity) from one mole of gaseous atoms to form one mole of gaseous positive ions.

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26
Q

Why is energy needed to remove electrons?

A

As electrons are negatively charged and protons in the nucleus are positively charged, there will be an attraction between them, so energy is required to pull the electrons away.

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27
Q

If an ionisation energy is positive what does this mean?

A

Ionisation energies are positive with the HIGHER the NUCLEAR CHARGE has a HIGHER ionization energy

28
Q

What evidence does first ionisation energy show?

A

Evidence for electrons being in sub shells and shells.

29
Q

What is electron affinity?

A

The AMOUNT of ENERGY needed to ADD ELECTRONS to atoms/ions.

30
Q

Definition for first electron affinity:

A

First electron affinity is the energy required to add one mole of electrons to one mole of gaseous atoms to form one mole of gaseous negative ions.

31
Q

Why are the first electron affinities negative?

What happens during the reaction?

A

Shows energy is released when an electron is added.. The more negative the electron affinity, the more stable the negative ion is that is formed.
Adding electrons to an atom is an EXOTHERMIC reaction so energy is given out to the surroundings.

32
Q

Explain the trends in the periodic table of the atomic size down a group and across a period.

A

Group- Increases. More energy shells filled with electrons so atom gets larger.
Period- Decreases- More electrons so stronger attraction between electrons and protons so atom is smaller.

33
Q

Explain the trends in the periodic table of the first ionisation energy down a group and across a period.

A

Group- Decreases because more energy levels so electrons in the highest energy level are further from the nucleus so require less energy to remove.
Period- Increase- More electrons so stronger attraction between electrons and protons so more energy needed to remove an electron.

34
Q

Explain the trends in the periodic table of the first electron affinity down a group and across a period.

A

Group- Becomes less negative because less energy given out when the atom and electron combines because more shielding between nucleus and outer electrons so more difficult for an electron to be attracted so only a small amount of energy released when both combine.
Small amount of energy given out because used a lot of energy (effort) to combine.
Period- Becomes more negative because more energy given out because it is easier to gain electrons. Electrons being added to the same shell and increasing proton number across the period so there is a stronger attraction between nucleus and outer electrons.

35
Q

What do Quantum numbers do?

A

Identify the various ENERGY LEVELS available within the atom in which the electron can reside.
Identification numbers: “address” for each electron in an atom by specifying the POSITION (or location) of an electron in an atom, predicting the DIRECTION of SPIN or rotation of the electron and determining the ENERGY and angular momentum of electron.

36
Q

What is an orbital?

A

An ORBITAL is a REGION of SPACE where there is a given probability of FINDING a particular ELECTRON.

37
Q

Principal Quantum Number (n)
What number is N always GREATER than?
What letters is n referred to by?
What shells contain multiple orbitals?

A 
0
n = 1 = K
n = 2 = L
n = 3 = M
n = 4 = N
Shells contain multiple orbitals except for n=1.
38
Q

Principal Quantum Number (n)

What happens in complex atoms, eg. more than one electron when n increases?

A

Energy levels get loser together.

39
Q

What does the quantum number “N” indicate?

A

DISTANCE of electron from NUCLEUS- Higher n, the further away the electron from nucleus.
ENERGY of ELECTRON- Higher n, higher energy electrons so less tightly held so easier to remove.
NUMBER of ELECTRONS a shell can hold- n can have 2n2.

40
Q

Principal Quantum Number (n)

How many electrons does each shell hold?

A

K-shell n =1 holds maximum 2×12 = 2 electrons
L-shell n = 2 2×22 = 8 electrons
M-shell n = 3 2×32 = 18 electrons
N-shell n = 4 2×42 = 32 electrons

41
Q

What does the principal quantum number “l” describe?

How do you work out l?

A

L describes the NUMBER of ORBITALS in a SUB SHELL as depending on the subshell the number of orbitals varies. Work out l by doing n-1, n-2 ect.

42
Q

What is a sub-shell?

A

A GROUP of ORBITALS with the same ENERGY.

43
Q

Principal Quantum Number (l)

What letters does the numbers of “l” correspond too?

A

Value of 0=s, 1=p, 2=d and 3=f.

44
Q

What does the quantum number “l” indicate?

A

Which sub shell an electron is in.
Energy of the sub shell – increases with increasing l.
Shape of the orbitals in that subshell.
Maximum number of electrons a given subshell can hold = 2(2l+1).

45
Q

L also shows the number of electrons in a sub shell. What are these numbers?

A

l is 0= s = 2 electrons
l is 1= p = 6 electrons
l is 2= d= 10 electrons
l is 3= f= 14 electrons

46
Q

L can be used to describe the shapes of sub levels- what are these shapes?

A

S orbital- Spherical
P orbital- Dumbell
D orbital- More complex
F orbital- Still more complex

47
Q

By using n and l what can be identified?

A

A particular subshell and therefore the location of an electron in the atomic energy levels.

48
Q

Examples of how n and l can be used to identify the location of an electron in the atomic energy levels.

A 
Shell, n, n- (1,2,3), l, Subshell "nl"
K, n=1, 1-1=0, l=0, Subshell= 1s
L, n=2, 2-1=1, l=1, Subshell= 2p
L, n=2, 2-2=0, l=0, Subshell= 2s
M, n=3, 3-1=2, l=2, Subshell= 3d
M, n=3, 3-2=1, l=1, Subshell= 3p
M, n=3, 3-3=0, l=0, Subshell= 3s
49
Q

What does the Principal Quantum Number (m) represent?

A

Represents the orbitals in a given sub-shell and does NOT indicate energy.

50
Q

What is the integral value ranging for “m”?

How do you find the total number of m values?

A

Ranging from –l through 0 to +l.

To find out the total number of m value is (2l+1).

51
Q

Principal Quantum Number (m)

Give examples of the values number of values for m in each sub shell (l).

A

l=0=s, m=0, 1 value, one s orbital.
l=1=p, m= -1,0,+1, 3 values, 3 p orbitals.
l=2=d, m= -2,-1,0,+1,+2, 5 values, 5 d orbitals.
l=3=f, m= -3, -2, -1, 0, +1, +2, +3, 7 values, 7 f orbitals.

52
Q

Principal Quantum Number (s)

How many numbers can ‘s’ have? Why?

A

2 numbers because an electron moving around the nucleus SPINS about its own axis either in a clockwise or anticlockwise direction so is either +1/2 or -1/2.

53
Q

How many electrons in 1 orbital?

A

2 electrons which have opposite spins.

54
Q

What is the clockwise and anticlockwise spinning position known as?
What does clockwise and anticlockwise spinning of electron produce?

A

Clockwise- ‘spin up’
Anti-clockwise- ‘spin down’

Opposite Magnetic Fields

55
Q

What is Heisenberg’s uncertainty principle?

A

You CANNOT determine the POSITION and MOMENTUM of an electron at the same time.

56
Q

What does the Aufbau Principle state?

A

Electrons enter the LOWEST available ENERGY LEVEL first.

57
Q

What does Hund’s rule of Maximum Multiplicity state?

A

When in orbitals of equal energy, electrons will try to remain UNPAIRED. Minimises repulsion between like charges, so the system is more stable.

58
Q

What does the Pauli Exclusion Principle state?

A

That no two electrons can have the same FOUR quantum numbers and only two electrons can go in each orbital, providing they are of opposite spin.

59
Q

What are the rules for the maximum number of electrons in energy levels in terms of n?

A 
n= Number of sub-levels
n2= Number of orbitals
2n2= Number of electrons in that orbital.
60
Q

What sub shell do you fill first which is out of the order? Why?

A

Fill 4s before 3d because 4s is lower in energy than 3d.

61
Q

What are the two special cases for writing electron configurations?

A

Chromium and Copper

62
Q

Electron Configuration of Chromium

A

1s2 2s2 2p6 3s2 3p6 4s1 3d5

63
Q

Electron Configuration of Copper

A

1s2 2s2 2p6 3s2 3p6 4s1 3d10

64
Q

What does a large jump between successive ionisation energy indicate?

A

A CHANGE in energy level from which the electron has been removed.

65
Q

What elements does MRI scanning image enhancement favour?

A

Elements with the most unpaired electrons.

Semester 1 Revision (9 decks)

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