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MCAT Chemistry 1 > Lesson 1 > Flashcards

Lesson 1 Flashcards

(72 cards)

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1
Q

Atomic Number

A

(Z) number of protons in nucleus, number of electrons in neutral atom

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2
Q

Isotopes

A

Atoms of subtle element (same atomic number) that differ in number of neutrons in nucleus (different masses)

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3
Q

Mass number

A

(A) combined number of protons and neutrons in a nucleus

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4
Q

Atomic mass

A

Average mass of all isotopes of an element

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5
Q

Binding energy

A

Smallest amount of energy required to remove a particle from a system of particles. Mass defect x speed of light squared

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6
Q

Nuclear strong force

A

Force that holds protons and neutrons together within an atomic nucleus, binding it together

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7
Q

Energy and Mass

A

Can be converted into each other (E=mc^2)

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8
Q

Electrostatic Force

A

Like charges repel

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9
Q

Strong Force

A

What holds nucleus together, is stronger than electrostatic forces which is how the nucleus stays together. Strong force only acts over short distances. Acts between all nucleons

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10
Q

Nuclear stability

A

Nuclear stability is when N/Z ratio = 1. Protons = Z. Neutrons = N. If N/Z ratio does not = 1. Nucleus is considered unstable. It is radioactive.

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11
Q

In nuclear equation

A

Nucleons and charge is conserved

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12
Q

Transmutation

A

Changing one element into another

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13
Q

Alpha decay

A

Proton being ejected. Represented by a Helium particle being ejected. Where 2 protons and 2 neutrons are being removed.

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14
Q

Beta decay

A

Where electron is being ejected. Proton is gained, neutron is lost.

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15
Q

Gamma decay

A

Charge and mass do not change. Atom goes from excited state to ground state by losing a gamma particle.

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16
Q

Positron Decay

A

Electron is ejected. Proton is being converted into neutron.

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17
Q

Half life

A

Time required for a certain amount of pure substance to fall to half its amount

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18
Q

How will proton behave in an electric field as compared to deuterium

A

Neither protium nor deuterium will accelerate

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19
Q

Which is stronger, the electrostatic force or the nuclear force? Why?

A

The nuclear strong force, because it overcomes the repulsion between protons to hold the nucleus together

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20
Q

Carbon has a half life of 5730 years and forms nitrogen 14 when it decays. Which type of decay causes this?

A

Beta decay

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21
Q

Beryllium 7 undergoes radioactive decay to form lithium 7. What type of decay is this?

A

Positron Emission

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22
Q

The half life of carbon 14 is 5730 years. If 40 grams of carbon 14 are allowed to decay, how much carbon 14 will remain after 14000 years?

A

7.4g

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23
Q

A radioactive sample is giving off gamma rays. What is occurring on the atomic scale?

A

A nucleus in an excited state releases a photo to return to its ground state

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24
Q

A researcher adds 5 g of NaCl to a beaker containing 120 g of water. How many water molecules are present?

A

4.0 x 10^24

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25
A researcher is looking to renovate his basement and is worried about radioactive isotopes. Upon investigation of his basement, he finds a large quantity of carbon 11, which is decaying into boron 11. Which of the following types of decay is this sample most likely undergoing?
Electron Capture.
26
Mass spectrometer
Works on the principles of separation ions based on their mass to charge ratio. (m/z) a sample is first ionised, creating cations. These ions are then accelerated by an electric field into a magnetic field, causing ions to follow curved paths based on their m/z.
27
What ions have the smallest radius in a mass spectrometer?
Ions that have a lower atomic mass will show to have the smaller radius in a mass spectrometer. (If all ions in question have the same charge)
28
What is a parent ion in a mass spectrometer?
The parent ion is what is produced when a compound is ionised. When the parent ion reaches the detector, it produces a parent peak.
29
What is the base peak?
The base peak is identified by the highest peak on the spectra graph. It is always made equal to 100% relative abundance.
30
Equation for magnetic force in terms of magnetic field strength and velocity of an ion
F=qvB
31
Why does an ion move in a circle in a mass spectrometer
Because magnetic force is perpendicular to the velocity of an ion
32
Photoelectric Effect
When a photon strikes a metal and results in the emission of an electron
33
What is the work function
Work function is the energy of the photon that was required in order to free the electron from the metallic surface
34
An electron’s total energy is composed of what two types of energy
Kinetic and electric
35
What equation can be used to determine the energy of any electron in terms of its quantum number
En=e1/n^2
36
An experimenter studying the photoelectric effect on a magnesium plate wants to increase the number of electrons ejected from the metal surface in a given amount of time. which of the following g changes should be made to achieve his goal? A) increase wavelength of photons B) decrease frequency of photons C) increase number of photons D) increase frequency of photons
Increase number of photons
37
What are the signs of kinetic and electric potential energy
Kinetic energy is positive, potential energy is negative
38
Heisenberg uncertainty principle
There is inherent uncertainty in the act of measuring a variable of a particle. Mainly in reference to position and momentum of a particle. Delta x multiplied by delta p is greater than or equal to plancks constant divided by 4 pi.
39
Principle quantum number
Main energy level occupied by an electron. Other name is shell.
40
Angular quantum number (l)
Shape of orbital.
41
Angular quantum number (l)
Shape of orbital.
42
Magnetic quantum number (ml)
Orientation of orbital. Ml = -l to l
43
Spin quantum numbers (ms)
The spin of the orbitals. Can be positive or negative 1/2. Positive means up, negative means down.
44
Diamagnetic
All electrons are spin paired and will be slightly repulsed by a magnetic field. NOBLE GASES ARE DIAMAGNETIC
45
Paramagnetic
Paramagnetic atom has some electrons that are not spin paired, and will be slightly attracted by an external magnetic field.
46
Aufbau principle
Building up principle. Electrons will fill in lower energy orbitals first.
47
Aufbau principle
Building up principle. Electrons will fill in lower energy orbitals first.
48
Pauli exclusion principle
Unique address principle. No two electrons can have the same 4 quantum numbers.
49
Hund’s Rule
Empty bus seat rule. Electrons will fill orbitals one at a time before pairing up.
50
Ionisation energy
Energy required to remove an electron from one mole of gaseous atoms to produce one mole of gaseous ions
51
Nuclear charge
More positive the charge In the nucleus, more attractive forces electron would feel
52
Effective nuclear charge
Nuclear charge - effect of shielding
53
Oxidation
Process when an atom has its oxidation state increase. Process of losing electrons.
54
Reduction
When an atom’s oxidation state is decreasing. Gain of electrons
55
Oxidising Agent
Chemical that is responsible for electrons being lost for another reactant.
56
Oxidising Agent
Chemical that is responsible for electrons being lost for another reactant.
57
Reducing Agent
Chemical that is responsible for gain of electrons in another reactant
58
Disproportionation
When a substance is being both oxidised and reduced in same reaction. Example - decomposition of hydrogen peroxide
59
Bronsted-Lowry Acid
Proton Donor. Has a conjugate base on other side of reaction.
60
Bronzed Lowry Base
Proton acceptor. Has a conjugate acid on other side of reaction.
61
Lewis Acid
Electron pair acceptor
62
Lewis Base
Electron Pair Donor
63
Lewis Base
Electron Pair Donor
64
Arrhenius Acids
Compounds that produce H+ ions in water
65
Arrhenius Bases
Substances that produce OH- ions in water
66
Equivalence point
Point in titration where number of moles of base added to an acid is equal to the number of moles of the acid
67
What is typically insoluble in water?
Carbonate and phosphate salts, unless they are bound to a group 1 or ammonium salt
68
What is typically insoluble in water?
Carbonate and phosphate salts, unless they are bound to a group 1 or ammonium salt
69
What is the pH of blood? Is it basic or acidic?
Blood is slightly basic, at 7.35 - 7.45
70
At the equivalence point, what is true about the oxidising and reducing agents in a redox reaction?
At the equivalence point the oxidising and reducing agents have both fully reacted.
71
Which Indicator should be used when titrating a strong acid with a strong base and why!
All 3 can be used because the titration curve for this reaction covers so many pH points
72
Polar aprotic solvent
Even though these solvents don’t have H atoms to donate. They can align their negative ends towards the positive charge in a polar molecule. I.e cyclic ethers in water

MCAT Chemistry 1 (1 decks)

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