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MCAT CHEMISTRY FLASHCARDS > MCAT CHEM CH. 4 > Flashcards

MCAT CHEM CH. 4 Flashcards

ATOMIC STRUCTURE AND PERIODIC TABLE

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1
Q

What is the smallest unit of any element?

A

Atom

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2
Q

All atoms have a central…?

A

Nucleus

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3
Q

What does the nucleus contain?

A

Protons and neutrons

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4
Q

What are the protons and neutrons in the nucleus known as?

A

Nucleons

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5
Q

Proton charge? Electron charge? Neutrons charge?

A

+, -, 0

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6
Q

The # of electrons outside the nucleus equals to…?

A

of protons inside the nucleus

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7
Q

How are the electrons held?

A

Electrostatic attraction of the + charged nucleus

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8
Q

What is the atomic #? Wha’s the symbol for it?

A

of protons in the nucleus of the atom, Z

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9
Q

What does the atomic # uniquely determines?

A

What element the atom is.

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10
Q

Where is Z demonstrated when noting an element?

A

Before the element, as a bottom left subscript

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11
Q

What is the relationship of the masses between the proton and the neutron?

A

A mass slightly more than one atomic mass unit

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12
Q

How much does 1 amu weigh?

A

1.66 X 10^-27

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13
Q

What is the mass of an electron?

A

About 0.05 percent he mass of either a proton or a neutron

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14
Q

All of the mass of an atom is due to its….?

A

Its nucleus

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15
Q

How do we calculate the mass number and what symbol is used to represent it?

A

of protons + # of neutrons in the nucleus of an atom, A

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16
Q

What is the formula for mass number?

A

A = Z + N

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17
Q

What does N represent in the equation A = Z + N?

A

Number of neutrons

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18
Q

How would we write Berylium if it had 5 neutrons? Based on subscript and superscript?

A

Superscript 9, Subscript 4, Be

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19
Q

What is an isotope?

A

Two atoms of the same element differ in their number of neutrons

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20
Q

How much does the nucleus occupy based on the atom’s size?

A

The nucleus occupies only the tiniest fraction of the atom’s volume

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21
Q

In other words,, all isotopes of a given element have….

A

The same atomic number but different mass numbers

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22
Q

An atom with 7 neutrons and a mass number of 12 is an isotope of what element?

A

Boron

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23
Q

What is the atomic weight of an element?

A

Weighted average of the masses of its naturally occurring isotopes

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24
Q

What is an example of an atomic weight of an element with various natural occurring isotopes?

A

Boron

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25
Q

What is an ion?

A

When a neutral atom gains or loses an electron and becomes charged

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26
Q

What is a negatively charged ion?

A

Anion

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27
Q

What is a positively charged ion?

A

Cation

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28
Q

What are protons and neutrons held tog ether by?

A

Strong nuclear force

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29
Q

Which force is stronger; nuclear force or electrical force between charged particles?

A

Nuclear force because it overcomes the electrical repulsion between the protons

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30
Q

What are unstable nuclei said to be?

A

Radioactive

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31
Q

What happens to radioactive nuclei?

A

Undergo transformations to make themselves more stable

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32
Q

What type of transformation can a radioactive nuclei undergo?

A

Altering the number and ratio of protons and neutrons or lowering their energy

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33
Q

What is the name of the process of lowering their energy?

A

Radioactive decay

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34
Q

What are the types of radioactive decay?

A

Alpha, beta and gamma decay

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35
Q

What is a parent nucleus?

A

The nucleus that undergoes radioactive decay

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36
Q

What is a daughter nucleus?

A

The resulting more stable nucleus

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37
Q

What does a large nucleus do in order to reduce the number or protons and neutrons?

A

Emits an alpha particle

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38
Q

What does the alpha particle consists of?

A

2 protons and 2 neutrons

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39
Q

How is the alpha particle denoted?

A

4 superscript 2 subscript alpha

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40
Q

What is the alpha particle equivalent to?

A

Equivalent to a helium-4-nucleus

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41
Q

How else can the alpha particle can be denoted?

A

superscript 4 subscript 2 He

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42
Q

What is the effect of alpha decay?

A

Reduces the parent’s atomic number by 2 and the mass number by 4

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43
Q

If polonium-210 has a superscript of 210 and a subscript of 84, what would it become?

A

Stable nucleus lead-206, superscript 206, subscript 82

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44
Q

What happens to the alpha particle that are emitted in high energy from the parent nucleus?

A

Energy is quickly lost as the particle travels through after of air

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45
Q

Due to the fact that the energy is quickly lost, how far does it travel?

A

Does not travel far and can be stopped by the outer layers of skin or a piece of paper

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46
Q

What are the three types of beta decay that exists?

A

B+, B- and electron capture

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47
Q

Each type of beta decay involves what?

A

The conversion of a neutron into a proton

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48
Q

What is the force used to complete the conversion of a neutron into a proton?

A

Weak nuclear force

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49
Q

Why particles are more dangerous, beta or alpha? Why?

A

Beta because they are less massive

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50
Q

Because beta particles are less massive, what do they have and what greater ability?

A

Have more energy and a greater penetrating ability

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51
Q

What are examples of stuff that can stop a beta particle?

A

Stopped by aluminum foil or a centimes of plastic or glass

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52
Q

What is called when an unstable nucleus covert a neutron into a proton and an electron?

A

B- particle

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53
Q

How is the atomic number of the resulting daughter nucleus based on B- decay?

A

1 greater than the radioactive nucleus but the mass number remains the same

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54
Q

What isotope is an example of radioactive nucleus that undergoes B- decay?

A

carbon-14

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55
Q

If the MCAT mention beta decay, what does it imply? How do you know that?

A

B- decay; it’s the most common type of beta decay

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56
Q

What is term for B+ decay?

A

Positron emission

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57
Q

What happens when an unstable nucleus contains too few neutrons?

A

It converts a proton into a neutron and a positron which is ejected

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58
Q

What is B+ decay?

A

Ejecting a positron; a proton converted into a neutron

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59
Q

What is the positron considered within the nucleus?

A

The electrons antiparticle

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60
Q

Why is the positron considered the electron’s anti-particle?

A

It’s identical to an electron except its charge is positive

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61
Q

What is the resulting daughter of nucleus based on B+ decay?

A

Daughter nucleus is 1 less than the radioactive parent nucleus but the mass number remains the same

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62
Q

What isotope is an example of radioactive nucleus that undergoes B- decay?

A

Fluorine-18

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63
Q

What is electron capture?

A

Increase number of neutrons by capturing an electron from the closest shell

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64
Q

From which shell is the electron capture taken from?

A

The n=1 shell

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65
Q

What is the electron used when taken from the closest shell?

A

Use it in the conversion of a proton into a neutron

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66
Q

What is the resulting daughter of nucleus based on electron capture?

A

Causes the atomic number to be reduced by 1 while the mass number remains the same

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67
Q

What is an example of electron capture?

A

Chromium-51

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68
Q

What happens to the nucleus after it undergoes alpha or any type of beta decay?

A

In an excited energy state

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69
Q

How can an excited nucleus go back to its ground state?

A

Emitting energy in the form of one or more photons of electromagnetic radiation

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70
Q

What are these photons referred as?

A

Gamma photons

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71
Q

Why can gamma rays penetrate anything easily?

A

They have neither mass nor charge

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72
Q

What type of surface will stop the gamma ray?

A

Few inches of lead or meter of concrete

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73
Q

What is the resulting daughter of nucleus based on electron capture?

A

Changes neither the atomic number nor the mass number of the nucleus

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74
Q

What example was used to show gamma decay?

A

Silicon-31

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75
Q

What is different between alpha/beta and gamma?

A

Alpha/beta change the identity of the nucleus, gamma does not

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76
Q

What does alpha decay do the the number of neutrons and protons?

A

Reduces number of protons ad neutrons

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77
Q

What does beta decay do the the number of neutrons and protons?

A

Decreases the number of neutrons, increases the number of protons

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78
Q

What does positron emission (beta plus) do the the number of neutrons and protons?

A

Increases the number of neutrons, deceases the number of protons

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79
Q

What does electron capture do the the number of neutrons and protons?

A

Increases the number of neutrons, deceases the number of protons

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80
Q

What does gamma ray do the the number of neutrons and protons?

A

Doesn’t change mass number or atomic number

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81
Q

What is a half-life?

A

The time it takes for 1 half-life some sample of the substance to decay

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82
Q

The shorter the half-life…..the….

A

The faster the decay

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83
Q

How does the amount of radioactive substance change overtime?

A

Radioactive substance decreases exponentially with time

84
Q

What is half-life denoted by?

A

t1/2

85
Q

What is the formula for exponential decay?

A

N = N0e^-kt

86
Q

What is the easiest way to write the exponential decay formula?

A

N = N0(1/2)^T/t1/2

87
Q

What does N mean in that formula? (N = N0(1/2)^T/t1/2)

A

The number of radioactive nuclei remaining

88
Q

What does T mean in that formula? (N = N0(1/2)^T/t1/2)

A

T is the total time the sample has decayed

89
Q

What does k mean in that formula? (N = N0e^-kt)

A

k is known as the decay constant

90
Q

What is the relationship with k and half-life?

A

k is inversely proportional to the half-life

91
Q

How would we calculate k if we only had the half-life equation?

A

k = (In2)/t1/2

92
Q

What is nuclear binding energy?

A

Energy released when the individual nucleons were bound together by the strong force to form the nucleus

93
Q

What would the nuclear binding energy equal to?

A

Energy required to break up the intact nucleus into individual nucleons

94
Q

The greater the binding energy….

A

the more stable the nucleus

95
Q

Why is the sum of the masses of all its nucleons individually greater than the combined nucleus?

A

Some mass is converted to energy when the nucleons bind together

96
Q

What is the difference between the energy loss mass during the nucleus binding the nucleons?

A

Mass defect, triangle mass

97
Q

The energy of the mass defect is equivalent to what?

A

Equivalent to the nuclear binding energy

98
Q

For stable nucleus, the mass defect would always be what?

A

Would always be positive

99
Q

How is the equation for mass defect?

A

Total mass of separate nucleons - mass of nucleus

100
Q

How is the nuclear binding energy denoted?

A

Eg

101
Q

How can the nuclear binding energy be found?

A

Using the Einstein’s equation for mass-energy equivalence

102
Q

What is Einstein’s equation for mass-energy equivalence?

A

Eg = (trianglem)c^2

103
Q

Based on Einstein’s equation for mass-energy equivalence, what does c represent?

A

C represents the speed of light, 3 X 10^8m/s

104
Q

What is the conversion factor between kg and joules?

A

1 kg = 9 X 10^16 J

105
Q

What is the nuclear domain and masses expressed in?

A

Atomic mass units

106
Q

What is the energy expressed in usually?

A

Electronvolts

107
Q

What is the conversion factor of an électronvolt?

A

1 eV = 1.6 X 10^-19 J

108
Q

How can the Einstein equation for mass-energy be converted into the eV units?

A

EB = (ineV) = [trianglem(in amu)] X 931.5 MeV

109
Q

What is an atom’s emission spectrum?

A

Energetic fingerprint that consists of a sequence of specific wavelengths and energies

110
Q

The energy of photons that are emitted are related to what?

A

Their frequencies and their wavelengths

111
Q

What is the equation of photon emission?

A

Ephoton = hf = hc/wavelength

112
Q

What does h refer to in the equation of photon emission equation?

A

Planck’s constant

113
Q

What is Planck’s constant?

A

6.63 X 10-34

114
Q

What does c refer to in the equation of photon emission equation?

A

Speed of light

115
Q

What was the model that Bohr proposed?

A

Electrons orbited the nucleus in circular paths

116
Q

What did Bohr mention about the distance from the electron to the nucleus?

A

Distance from the nucleus was related to the energy of the electrons

117
Q

Electrons with greater amounts of energy orbited the nucleus at……..

A

greater distance

118
Q

What can electrons in the atom not assume based on energy and what’s the correct term?

A

Cannot assume arbitrary energy but have quantized energy states

119
Q

What does having quantized energy states means for the electrons orbits?

A

Can only orbit at certain allowed distances from the nucleus

120
Q

How can an electron jump to a higher level?

A

If an electron absorbs energy that’s exactly equal to the difference in energy between its current level and of its higher level

121
Q

How can an electron drop to a lower energy level?

A

By emitting a photon with an energy exactly equal to the difference between the levels

122
Q

The Bohr predicted what kind of spectra?

A

Line spectra

123
Q

What is the ground state represented by? And what does it mean?

A

n=1, lowest possible energy level

124
Q

What is the excited state?

A

Jumps to a higher energy level

125
Q

What are Bohr atoms?

A

Atoms or ions containing one electron

126
Q

What is the Bohr atom equation?

A

En = (-2.178X10^-18) / n^2

127
Q

When there is a smaller energy change level, the wavelength would be…..

A

Of longer length because they are inversely related

128
Q

What does the Bohr model fail to demonstrate?

A

The electron-electron interactions that exist in many-electron atoms

129
Q

What do the quantum numbers designate?

A

Designating shell, sub shell, orbital and spin

130
Q

What is the energy shell of an electron represented by?

A

n

131
Q

What is an energy sub shell?

A

One or more orbitals that describe the shape and energy of the orbitals

132
Q

Based on quantum theory, what is an orbital?

A

Three-dimensional region around the nucleus in which the electron is most likely to be found

133
Q

What are the denoted letters for subshells?

A

s, p, d or f

134
Q

Each higher energy shell contains what?

A

One additional subshell

135
Q

If the first energy shell contains he s subshell, what would the second energy shell contain?

A

Both the s and p subshell

136
Q

What are degenerate orbitals?

A

Subshell containing one or more orbitals of the same energy

137
Q

How do the number of orientations differ between subshells?

A

The number of orientations increases by two in each successive sub shell

138
Q

What is an example of different orientations for subshells

A

The s sub shell contains one orientation and the p subshell contains three orientations

139
Q

Each electron has how many possible spin states?

A

Two

140
Q

What can the two spin states be considered?

A

Can be considered the electron’s intrinsic magnetism

141
Q

Because an electron has two possible spin states, how many electrons can an orbital have as max?

A

Two electrons

142
Q

What are the spins of the two electrons in the orbital?

A

One spin-up, one spin-down

143
Q

What do we say if an orbital is full?

A

The electrons it holds are “spin-paired’

144
Q

What are the three basic rules of electron configurations?

A
  1. Electrons at lowest energy orbitals valuable
  2. Electrons occur available orbitals singly before pairing
  3. No more than 2 in any given orbital
145
Q

What is the Aufbau principle?

A

Electrons occupy the lowest energy orbitals available

146
Q

What is the Hund’s rule?

A

Electrons in the same sub shell occupy available orbitals singly, before pairing up

147
Q

What is the Pauli exclusion principle?

A

There can be no more than two electrons in any given orbital

148
Q

What is the electron configurations Oxygen?

A

1s^2 2s^2 2p^4

149
Q

What is a complete octet and which types of elements have them?

A

8 valence electrons are in filled subshells and the noble gases

150
Q

What are the noble gases trait related to having a full octet?

A

Chemical stability and lack of reactivity

151
Q

What is. diamagnetic?

A

An atom that has all of its electrons spin-paired

152
Q

What are the required factors of a diamagnetic?

A

Contain an even number of electrons; have all of its occupied subshells filled

153
Q

How is the magnetic field for diamagnetic atom and why?

A

Magnetic fields they create dance and leave no net magnetic field behind since they are spin-paired

154
Q

Since there is no magnetic field, what happens to an atom that is diamagnetic?

A

Will be repelled by an externally produced magnetic field

155
Q

What is a paramagnetic atom?

A

Atom’s electrons are not all spin-paired

156
Q

When an external magnetic field is produced, what’s the reaction of paramagnetic atoms?

A

Attracted

157
Q

What is a period in a periodic table?

A

A period is each horizontal row to the periodic table

158
Q

What is a group or family in a periodic table?

A

Each vertical column

159
Q

What are the anomalies to the electron configurations rule?

A

Atoms can achieve a lower energy stately having a filled or half-filled d sub shell

160
Q

What example of atoms are anomalies to the EC rule?

A

Chromium and same family, Copper and same family

161
Q

What does it mean to be isoelectronic? Provide examples?

A

Atoms that gain electrons put them in the first available orbital; example: Neon and F-

162
Q

When transition metals lose electrons, from which orbital do they lose it first?

A

They lose it from the s orbital before losing it from the d

163
Q

Where are transition metals located in the periodic table?

A

Elements in the d block

164
Q

What is the definition of an excited state?

A

When electron has jumped to a higher energy level

165
Q

When an electron turns into an excited state, does it change the amount of electrons from the atom?

A

No, they stay the same amount of electron, just jumped to a higher energy level orbit

166
Q

What’s the name of group 1 in a periodic table?

A

Alkali metals

167
Q

What’s the name of group II in the periodic table?

A

Alkaline earth metals

168
Q

What’s the name of group vii in the period table?

A

Halogens

169
Q

What’s the name of group viii in the periodic table?

A

Noble gases

170
Q

What are the d block elements considered?

A

Transition metals

171
Q

What are the s and p blocks elements considered?

A

Representative elements

172
Q

What are the f block elements considered?

A

Rare earth metals

173
Q

What are alkali metals and alkaline earth metals usually used as in redox reactions?

A

Reducing agents to lose valence electrons in order to get a stable octet

174
Q

What do halogens usually exist as and why?

A

As a diatomic molecule (Fsubscript2) where one electron of each atom is shared
Why: Only require a single electron to achieve a stable octet

175
Q

How do halogens behave in redox reactions?

A

Powerful oxidizing agents - gain electrons

176
Q

What’s the valence configurations for alkali metals?

A

ns1

177
Q

What’s the valence configuration for alkaline earth metals?

A

ns2

178
Q

Whats the valence configuration for halogens?

A

ns2np5

179
Q

What’s the valence configuration for noble gases?

A

ns2np6

180
Q

What are the elements that possess both metals and nonmetals qualities called?

A

Metalloids

181
Q

Where are metalloids found in the periodic table?

A

Diagonal from B to Po

182
Q

What is the shielding effect or nuclear shielding?

A

Each filled shell between the nucleus and valence electrons shields valence electrons from the full effect of the protons in the nucleus

183
Q

What is Zeff?

A

The reduced electrical pull from the protons due to the negative charges of the electrons in the filled shells in between

184
Q

When the amount of protons increase…..

A

Their total pull on the outermost electrons increases too

185
Q

As you move from left to right in the periodic table, what happens to the elements?

A

The atomic radius decreases

186
Q

Why does the atomic radius decreased from left to right?

A

Electrons are being added but no new shell so valence electrons feel a stronger pull

187
Q

Why does atomic radius increased from top to bottom when going down a group?

A

Increase shielding causing less tightly bound since they geed a smaller effective nuclear charge

188
Q

As you move from top to bottom in the periodic table, what happens to the elements?

A

The atomic radius increases

189
Q

What happens to a cation atomic radius?

A

Decrease because as e-‘s are removed, the ones left are closely pulled in

190
Q

What happens to an anion atomic radius?

A

Increases

191
Q

What is the atom’s first ionization energy (IE)?

A

The amount of energy necessary to remove the lest tightly bound electron from an isolated atom

192
Q

What happens to the ionization energy when you move from left to right across a period?

A

Increases because the valence electrons are more tightly bound

193
Q

What happens to the ionization energy when you move from bottom to up across a period?

A

Increases because the valence electrons are more tightly bound

194
Q

What is the second ionization energy of an atom? (IE2)

A

The energy required to remove the least tightly bound electron from the cation X+

195
Q

What is electron affinity?

A

The addition of an electron to an isolated atom

196
Q

What is electron affinity negative?

A

IF energy is released when the electron is added

197
Q

When is electron affinity positive?

A

If energy is required to add the electron

198
Q

What type of electron affinity does halogens have and why?

A

Large negative; the addition of an electron would give them their octet

199
Q

What type of electron affinity does noble gases have and why?

A

Positives because the added electron begins to fit a new level and destabilizes the electron configuration

200
Q

Which types of elements have positive electron affinity?

A

Nobles gases and alkaline earth metals

201
Q

What is the electron affinity trend on the periodic table?

A

Decrease left to right, decreased bottom to up

202
Q

What is electronegativity?

A

A measure of an atom’s ability to pull electrons to self when it forms a covalent bond

203
Q

The greater the tendency to attract electrons…..

A

The greater the atom’s electronegativity

204
Q

What is the elements you have to remember their electronegativity?

A

F > O > N = Cl > Br > I > S > C = H

205
Q

What is the periodic trend of electronegativity?

A

Increases from left to right, increases from bottom to top

206
Q

What is acidity of an atom?

A

How well a compound donates protons, accepts electrons or lowers pH in a chemical system

207
Q

What is the periodic table trend of acidic elements?

A

Increases from left to right, decreases bottom to up

MCAT CHEMISTRY FLASHCARDS (4 decks)

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