Atomic Structure & Periodic Table Flashcards

0
Q

Neutral atoms have…

A

The number of electrons outside the nucleus is equal to the number of protons inside the nucleus. Electrons are held in the atom by the electrical attraction of the positively charged nucleus

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1
Q

What is an Atom?

A

The smallest unit of any element. All atoms have a central nucleus which contains protons and neutrons known as nucleons. Each proton has an electric charge of +1; neutrons have no charge. Outside the nucleus are electrons each have an electric charge of -1

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2
Q

What is the atomic number of an atom?

A

Symbol= Z
Number of protons
Shown in a subscript before the element

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3
Q

Mass of proton and neutron

An electron?

A

Each have a mass slightly more than one atomic mass unit (1 amu =1.66x10^-27 kg)
An electron has a mass that’s only 0.05% the mass of either a proton or a neutron
All the mass of an atom is due to the nucleus

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4
Q

Atomic mass equals

A

A=Z+N

Atomic mass is written as a super sub script before the elements

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5
Q

Isotopes

A

If two atoms of the same element differ in their numbers of neutrons they are called isotopes.
This affects only the mass number.

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6
Q
And item would seven neutrons and a mass number of 12 is an isotope of what element?
A. Boron
B. Nitrogen
C. Magnesium
D. Potassium
A

A. Boron
A equals 12
N equals 7
So Z would equal 5 which is the atomic number
Remember the atomic number is not affected in an isotope

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7
Q

Are elements found in their one form in nature?

A

Elements exist naturally as a collection of the isotopes. The atomic weight of an element is a weighted average of the masses of its naturally occurring isotopes.
In order to get the weighted average the isotopes are multiplied by the percentages which they occur in the natural world and then added
Atomic weight of an element or the weighted average is found on the periodic table

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8
Q

What are ions?

A

What a neutral atom gains or loses electrons, it becomes charged, and the resulting atom is called an ion.
For each electron it gains, and atom acquires a charge of -1 unit, and for each electron it loses an atom acquires a charge of a +1 unit. A negatively charged ion is called an anion, while a positively charged ion is called a cation.

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9
Q

What is the strong nuclear force?

A

Protons and neutrons in the nucleus are held together by force called the strong nuclear force. It is stronger than the electrical force between charged particles, since for all atoms besides hydrogen, the strong nuclear force must overcome the electrical repulsion between the protons.
In fact, of the four fundamental forces of nature, the strong nuclear force is the most powerful even though it only works over extremely short distances.

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10
Q

Unstable nuclei are?

A

Said to be radioactive, and they undergo a transformation to make them more stable altering the number and ratio of protons and neutrons or just lowering their energy.
Such a process is called radioactive decay, and there are three types alpha, beta, and gamma.
The nucleus that undergoes radioactive decay is known as the parent.
And the resulting more stable nucleus is known as the daughter.

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11
Q

What are the three types of radioactive decay?

A

Alpha, beta, gamma

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12
Q

What is alpha decay?

A

When a large nucleus wants to become more stable by reducing the number of protons and neutrons, it emits an alpha particle.
An alpha particle, denoted by 4/2 (alpha sign), consist of two protons and two neutrons.
Alpha decay reduces the parents atomic number by 2 and the mass number by 4

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13
Q

Polonium-210 decaying to it’s more stable form as lead-206 is an example of what type of decay?

A

Alpha decay.

it is an alpha-emitter

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14
Q

What magnitude of energy do alpha particles emit from the parent nucleus?

A

High energy.
This energy is quickly lost as the particle travels through matter of air. As a result the particles do not typically travel far, and can be stopped by the outer layers of human skin or a piece of paper.

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16
Q

What is beta decay?

A

There are three types of beta decay: β-, β+, and electron capture. Each type of beta decay involves the conversion of a neutron into a proton, or vice versa, through the action of the week nuclear force.
Beta particles are more dangerous than alpha particles since they are significantly less massive. They therefore have more energy and a greater penetrating ability. However, they can be stopped by aluminum for foil or a centimeter of plastic or glass

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17
Q

β- Decay

A

When an unstable nucleus contains too many neutrons, it may convert a neutron into a proton and an electron (which is also know as a beta- particle) which is ejected.
The atomic number of the resulting daughter nucleus is 1 greater than the radioactive parent nucleus, but the mass number remains the same.
The isotope carbon – 14, the decay of which is the basis of radiocarbon dating of archaeological artifacts, is an example of a radioactive nucleus that undergoes beta- decay
14/6C —–> 14/7C (0/-1 beta is ejected)
This is the most common beta decay so if mentioned on MCAT WITHOUT SPECIFICATION, it’s beta-

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17
Q

Electron capture

A

Another way for an unstable nucleus to increase its number of neutrons is to capture an electron from the closest electron shell (the n=1 shell) and use it in the conversion of a proton into a neutron.
Just like positron emission, electron capture causes the atomic number to be reduced by 1 while the mass number remains the same.
51/24Cr + 0/-1e- —–> 51/23V
(Loses proton because it’s converted into neutron)

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18
Q

β+ Decay

A

Also know as Positron Emission
When an unstable nucleus contains too few neutrons, it converts a proton into a neutron and a positron, which is ejected. This is known as Beta+ decay.
-The positron is the electron’s anti-particle; it’s identical to and electronics at its charge is positive.
–The atomic number of the resulting daughter nucleus is 1 less than the radioactive parent nucleus, but the mass number remains the same.
18/9F—-> 18/8O. (0/+1 beta ejected)

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19
Q

Gamma decay

A

A nucleus in an excited state—which is usually the case after a nucleus has undergone alpha or any type of beta decay— can “relax” to its ground state by emitting energy in the form of one or more photons of electromagnetic radiation. These photons are called Gamma photons (symbolized by gamma symbol y) and have a high frequency and energy.
Gamma photons or gamma rays have neither mass nor charge, and can therefore penetrate matter most effectively. A few inches of lead or about a meter of concrete. Most Scana race there each action from a radioactive Adam changes neither the atomic number nor the mass number of the nucleus.
31/14Si–beat neg. D–> 31/15P*—gamma D–>31/15P+0/0y emitted
* means in excited stage
Alpha and beta decay changes the identity of the element, gamma doesn’t. Gamma decay is simply the expulsion of energy.

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20
Q

What happens during gamma decay?

A

Brings an excited nucleus to a lower energy level, doesn’t change mass number or atomic number.

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21
Q

What happens during alpha decay?

A

Decreases the number of neutrons and protons in large nucleus, subtract 4 from the mass number and subtract 2 from the atomic number.

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22
Q

What happens during positron emission?

A

Increases the number of neutrons, decreases the number of protons, and subtract 1 from the atomic number.

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23
Q

What happens during β- decay?

A

Decreases the number of neutrons, increases the number of protons, and adds 1 to the atomic number.

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24
Q

What happens during electron capture?

A

Increases the number of neutrons, decreases the number of protons, subtract 1 from the atomic number.

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25
Q

Americium-241 is used to provide intracavitary radiation for the treatment of malignancies. This radioisotope is known to undergo alpha decay. What is the daughter nucleus?

A

247Np

Alpha decay reduces atomic mass by 4 and atomic number by 2

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26
Q
Radioactive calcium-47, a known β-  emitter, is administered in the form of 47CaCL2 by IV as a diagnostic tool to study calcium metabolism. What is the daughter nucleus of 47Ca?
    A. 46K
    B.  47K
    C.  47Ca+
    D.  47Sc
A

D. 47Sc

Adds 1 proton and atomic weight doesn’t change.

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27
Q

Vitamin B12 can be prepared with radioactive cobalt (58Co), a known bet+ emitter, and administered orally as a diagnostic tool to test for defects in intestinal vitamin B12 absorption. What is the daughter nucleus of 58Co?

A. 57Fe
B. 58Fe
C. 59Fe
D. 59Ni

A

B. 58Fe

Reduces atomic mass by 1 but atomic weight stays the same

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28
Q

A certain radioactive isotope is administered orally as a diagnostic tool to study pancreatic function and intestinal fat absorption. This radioisotope is known to undergo beta- decay, and the daughter nucleus is xenon – 131. What is the parent radioisotope?

A. 131Cs
B. 131I
C. 132I
D. 132Xe

A

B. 131I

Since xenon-131 is the daughter we are reversing the process. Instead of adding a proton to atomic number, subtract 1 proton to get the parent.

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29
Q

which mode of radioactive decay causes change in the mass number of the parent nucleus?

A

Alpha decay

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30
Q

One of the naturally occurring radioactive series begins with radioactive 238U. It undergoes a series of decays, one of which is: alpha, beta, beta, alpha, alpha, alpha, alpha, alpha, beta, beta, alpha, beta, alpha, beta. What is the final resulting nuclide of the series of decays?

A. 204Pb
B. 204Pt
C. 206Pb
D. 206Pt

A

C. 206Pb

Alpha: -4/-2
Beta-: 0/+1

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31
Q

What is a half-life?

A

Different radioactive nuclei decay at different rates. The half-life, which is denoted by t1/2, of a radioactive substance is the time it takes for one-half of some a sample of the substance to decay.
Thus, the shorter the half-life, the faster the decay. The amount of radioactive substance decreases exponentially with time.

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32
Q

The shorter the half-life….

A

The greater the decay constant, and the more rapidly the sample decays

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33
Q

Cesium-137 has a half-life of 30 years. How long will it take for only 0.3 g to remain from a sample that had an original mass of 2.4 g?

A

90 years

2.4–30yrs–> 1.2–30yrs–> .6–30yrs–>.3

30x3=90

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34
Q

If 58Ca has a half-life of 72 days, approximately what percentage of the radioisotope will still remain in the patient after a year?

A. 3%
B. 5%
C. 8%
D. 10%

A

A. 3%

360 days/72 days=5 half-lives
(1/2)^5 equals 1/32 of the original amount administered.
1/32—>3/100 about 3%

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35
Q

Iodinated oleochemicals acid, containing radioactive iodine-131, is administered orally to study a patient’s pancreatic function. If 131I has a half-life of 8 days, how long after the procedure will the amount of 131I remaining in the patient’s body be reduced to 1/5 it’s initial value?

A. 19 days
B. 32 days
C. 40 days
D. 256 days

A

A. 19 days

1/5 is between 1/4 and 1/8
1/4=25%=2t
1/8=12.5%=3t
So about 2 half-lives occurred, so 8 days times 2 is 16.

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36
Q

What is the usual half-life percentages of remaining substance?

A
Time.                      Amount remaining
t(1/2)=1 half-life.      1/2=50%
t(1/2)=2 half-life.       1/4=25%
t(1/2)=3 half-life.      1/8=12.5%
t(1/2)=4 half-life.      1/16=6.25%
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37
Q

What is an Emission Spectrum?

A

A glass filled with a small sample of an element in gaseous form. When electric current passed through the glass, the gas begins to glow with a color characteristic of that particular element.
If the light emitted by the gas is then passed through the prism, which will separate the light into it’s compliment wavelengths
Basically shows which wavelengths are emitted by the element.
The emission spectrum gives an energetic fingerprint of the element because it consists of a unique sequence of bright lines that correspond with the specific wavelengths and energies.

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38
Q

What are the different ways an electron that is in excited say can “relax” or jump back down to ground state (its original state)?

A

It can either 1) drop down in smaller increments, for example excitation=n=3, drops down to n=2. This will give you the exact energy difference between n=3 and n=2
2) drop down directly to ground state, for example excitation=n=3, drops down to n=1, gives energy difference between n=3 and n=1.

39
Q

What is the equation relating photons (particles of light) that are emitted to their frequencies and wavelengths?

(Emission spectrum)

A
E(photon)=hf=c/λ
  or E(photon)=h x c/λ
f=frequencies 
λ=wavelength
h=universal constant called Planck's constant (6.63x10^-34 J*s)
C=speed of light
40
Q

The Bohr Model of the Atom

A

By using the emission spectrum, Niels Bohr was able to create a new model, one with energy levels. He theorized that electrons in the atom orbited the nucleus in circular paths, distance from the nucleus was related to the energy of the electrons, and the electrons with greater amounts of energy orbited the nucleus at greater distance.
Electrons cannot assume an arbitrary energy but have quantized energy states.
By observing the energy spectrum of particular elements, he was able to discern the energy levels of atoms.
1) When the electrons emits the wavelengths passing through, it’s dropping back to normal level after excitation. The emission of energy=difference between the two energy levels.
2) The amount of energy that electron absorbs is equal to the amount of energy it takes to be in the energy levels the electron jumps up to due to excitation.
(Specific energy corresponds to specific wavelength–able to see this due to color of wavelength once separated in line spectra)
*remember this is modeled by Hydrogen

41
Q

Calculating energy level equation

A

E=(-2.178 x 10^-18)/n^2

Example: E(3–>1)=(-2.178 x 10^-18J)/(1^2) - (-2.178 x 10^-18 J)/(3^2)
E(3–>1)= -1.936 x 10^-18 J
*Note, the calculation is negative because it is energy being released from the electron. If it is positive, it means the energy is absorbed by the electron.

42
Q

What is a Bohr Atom?

A

An atom that has only one electron

43
Q

Which of these is NOT an example of a Bohr atom?

A. H
B. He+
C. Li2+
D. H+

A

D. H+

Bohr’s atom only should have one electron

44
Q

Once you calculate the energy with Bohr’s equation, how can you find the wavelength of the photon?

A

Use E=h x c/λ

45
Q

Are you able to see all electron transitions produced by photons?

A

No, some you cannot see with the naked eye, but all transitions in an atom will produce photons either in the ultraviolet, visible, or infrared region of the electromagnetic spectrum.

46
Q

What happens to the wavelength if the energy change from one level to another in the atom changes?
When the energy change is smaller?
When the energy changer is larger?

A

Wavelength and energy change are inversely related meaning if the energy change is smaller, the wavelength is longer, and when the energy change is bigger, the wavelength is shorter.

E=h x c/λ

47
Q

The Quantum Model of the Atom

A

Is the official model we use to this day because the Bohr model, although it predicted the atomic spectra of one electron atoms accurately, didn’t do a good job at predicting the atomic spectra of many-electron atoms accurately.
We still believe Bohr’s hypothesis that there are energy levels but this model furthers the hypothesis by developing 4 quantum numbers to establish the ‘locations’ and depict electron interactions more accurately.
4 quantum numbers: shell (n), subshell, orbital, and spin.

48
Q

Quantum Number: What is the Energy Shell (n) of an atom?

A

Resembles the circular orbitals in Bohr’s model.

An electron in the higher shell has a greater amount of energy and a greater average distance from the nucleus.

49
Q

Quantum Number: What is the Energy Subshell of an atom?

A

This mainly deals with the probability of finding an electron in a certain area, or the shape of the orbital. An orbital describes a three-dimensional region around the nucleus in which the electron is most likely to be found. (Remember, the movement of electrons resembles the movement of waves)
A subshell in an atom is comprised of one or more orbitals and is denoted by a letter (s, p, d, f) that describes the shape and energy of the orbital(s).
This describes the shape of the orbital
The orbitals get progressively more complicated has the energy levels increases. Each energy level contains more subshells as you go higher. For example n=1 has only s while n=2 has both s and p subshells.

50
Q

Quantum Number: What is the Orbital Orientation of an atom?

A

This mainly deals with how many orbitals (orientations) are in a subshell. The one or more orbitals of the same energy in a subshell are refered to as degenerate orbitals.
The number of orbitals increases by 2 with every different orientation/subshell.
For example, s subshell only contains 1 orientation while the p subshell as 3 orientations. d has 5 and f has 7

51
Q

Quantum Number: What is the Electron Spin in an atom?

A

Every electron has two possible spin state, which can be considered the electron’s intrinsic magnetism.
Because of this every orbital can accommodate up to 2 electrons, with one spin-up and one spin-down.
If the orbital is filled, the electrons it holds are “spin-paired.”

52
Q

What is Hund’s Rule?

A

Electrons in the same subshell must occupy the available orbitals singly before pairing up. Spins must all be in the same direction.

53
Q

What is the Pauli Exclusion Principle?

A

No more than two electrons allowed in each orbital.

54
Q

What is Aufbau Principle?

A

You must fill the lowest energy shell first then work your way up.

55
Q

What is a complete octet?

A

The noble gases have this, where the eight valence electrons fill the last subshells, making it neutral (or very difficult to create chemical interactions since the elements are content). Accounts for chemical inactivity.
Pattern: the eight valence electrons fill in the last (n)s and (n)p (usually it’s the first p orbital).
All other elements strive for this complete octet.

56
Q

What is a diamagnetic atom?

A

When all of its electrons are spin-paired.
(so must contain an even number of electrons and have all of its subshells occupied.
Since all are spin-paired, there is no net magnetic field due to the individual magnetic fields canceling out.
Such an atom will be repelled by an externally produced magnetic field.

57
Q

What is a paramagnetic atom?

A

When it doesn’t have all of its electrons spin-paired. They are attracted into externally produced magnetic fields.

58
Q

Periodic Table: What is a group?

A

Also known as family. It is the vertical column.

-It can tell you where the outermost valence electrons are (which orbital: s, d, p, or f)

59
Q

Periodic Table: What is a period?

A

It is the horizontal row.

-It can tell you what shell (energy level) the outermost electrons occupy.

60
Q

Periodic Table: In order to tell what shell the electrons of a d-block fill, what do you do with n?

A

n-1
for example, 4s2 3d1
also refer to the electron filling diagram

61
Q

Are there exceptions to the rules for electron configuration? If so, name examples.

A

Yes, because some elements can achieve a lower energy state (higher degree of stability) by having a half filled d-subshell.
For example, Chromium (Cr, Z=24), you would think its electron configuration would only have four electrons in the d orbital but it would be more stable if it had 5, so it promoted one of its electrons from the s orbital to go up to make it 5. Configuration: Ar 4s1 3d5
Another example: Copper (Cu, Z=29) is actually 4s1 3d10 because it has more stability if d is filled.
Other elements that display the same behavior are Mo (molybdenum), Ag (silver), and gold (Au).

62
Q

What is the electric charge of an ion?

A

It is a nonzero charge.

63
Q

What is an anion?

A

An atom that has more electrons than protons.

Negative

64
Q

What is a cation?

A

An atom that has less electrons than protons.

Positive

65
Q

What does isoelectronic mean?

A

It means that two elements are the same in electron configuration after one of the elements becomes an ion, which changes their electron configuration.

66
Q

How do you calculate the electron configuration of an ion?

A

Simply move to the right or left of the periodic table to see which element it is isoelectronic with. Right=anion, left=cation

67
Q

Electrons that are removed from the atom, always come from the…

A

valence shell (these electrons are the first to go)

68
Q

How can calculating the new electron configuration for a transition metal that became an ion be different?

A

Remember, there is a different order of filling for the d-block. It will lose its electrons from the s block first before it loses from the d because the d block is still higher in energy despite it being on a lower energy level than the s.
Example: 4s2 3d2—> 4s1 3d2 (cation)

69
Q

Any electron configuration of an atom that is not as you would assign it, would mean what?

A

It is in it’s excited state. Meaning that one electron was promoted to the next level.

70
Q

Alkali Metals

A

Group 1

(n)s1

71
Q

Alkaline Earth Metals

A

Group 2

(n)s2

72
Q

Halogens

A

Group 7

(n)s2 (n)p6

73
Q

Noble Gases

A

Group 8

(n)s2 (n)p6

74
Q

Transition Metals

A

d-block

75
Q

Representative Metals

A

s and p blocks

77
Q

Rare Earth Metals

A

f block

78
Q

The chemical reactivity is determined by the what?

Give examples of each group.

A

Determined by the electron configuration, or how many valence electrons there are.
The noble gases are the most stable because they have a full octet.
The Halogens are closer to stability but need one more electron to complete octet. So highly electronegative. You will see them normally in diatomic molecules (covalent bond). When in a compound with another element, they behave as powerful oxidizing agents (gaining electrons). They become stable either as X- anions or sharing electrons with other nonmetals.
The alkali metals and alkaline earth metals possess one or two electrons, meaning they want to lose them, behaving as reducing agents in reactions. Generally X+ or X+2 cations.

79
Q

List the Periodic Trends

A

Shielding, atomic and ionic radius, ionization energy, electron affinity, electronegativity, acidity

80
Q

Periodic Trend: What is shielding?

A

Each filled shell between the nucleus and the valence electrons shields (or protects) the valence electrons from the full effect of the positively charged protons in the nucleus. (This means it is easier for the atom to lose these electrons or for reactions to occur).
This is called nuclear shielding or shielding effect.
Where the positive charged pull of the protons is reduced by the negative charges of the electrons in the filled shells.
Result: reduction in the positive elementary charge, from Z to Z(eff) (for effective nuclear charge)

81
Q

What are the forces that influence a solitary He atom?

A

Electrostatic attraction between the electrons and nuclear protons.
Electrostatic repulsion between the electrons

82
Q

Periodic Trend: What is atomic and ionic radius and how is it a factor in periodic trend?

A

Move from left to right (period): atomic radius decreases due to the number of protons increasing across the period but the number of shells remaining the same (only changes in the beginning of each period), so the electrons are being pulled in tighter to the atom due to the greater effective nuclear charge (of the protons).
Move down a group: atomic radius increases due to the number of shells increasing making the radius larger and adding more shielding effect so the valence electrons can venture a little more (feeling less effective nuclear charge).
Bigger the atom, the easier it loses electrons.

83
Q

What would happen to the radius if you wanted to create an anion?
A cation?

A

Anion: removes electrons, so radius gets bigger (ones that are left are drawn in more closely)
Cation: adds electrons, so radius gets smaller
X+<X-

84
Q

Periodic Trend: What is Ionization Energy?

A

The energy it takes to remove an electron.

85
Q

Periodic Trend: What is an atom’s First Ionization Energy?

A

The amount of energy it takes to remove the least tightly bound electron from an atom.
Symbol: IE OR IE1

86
Q

Periodic Trend: What is an atom’s Second Ionization Energy?

A

The amount of energy it takes to remove the least tightly bound electron from a cation, X+. IE2 will always be greater than IE1. It takes more energy to remove an electron the second time because the radius for a cation is smaller due to the increase in effective nuclear charge.

87
Q

Periodic Trend: What is the periodic trend for Ionization Energy?

A

Increases as you go across the table (since the valence electrons are more tightly bound, meaning it takes more energy to get them away)
decreases as you go down.
Ionization energy for noble gas will always be very large.

88
Q

Periodic Trend: What is Electron Affinity?

A

The energy associated with the addition of an electron to an isolated atom. It can either be defined as positive or negative.
Positive Electron Affinity: energy is required to add an electron.
Negative Electron Affinity: energy is released when the electron is added. (meaning the atom as become more stable by adding an electron)
Example: Halogens have a large negative electron affinity because adding that one electron will make it an octet making it more stable (releasing energy), but adding an electron to the noble gases or alkali/alkaline earth metals would make them destabilized anions, thus positive.

89
Q

Periodic Trend: What is the periodic trend for Electron Affinity?

A

Increases in negativity as you go across the table (exception of noble gases)
decreases in negativity as you go down a group (exception of noble gases)

90
Q

Periodic Trend: What is Electronegativity?

A

A measure of an atom’s ability to pull electrons to itself when it forms a covalent bond. Basically, it is the greater attraction is has for electrons in a shared bond.
This is why the electrons in a compound will tend to be more associated with one atom over another, thus creating the polar covalent bond, the one having the greater electronegativity being polar.

91
Q

Periodic Trend: What is the periodic trend for Electronegativity?

A

Left to right: increases

Down a group: decreases

92
Q

What is the order of electronegativity for the nine more electronegative elements?

A

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

93
Q

Periodic Trend: What is the Acidity of an atom?

A

The measure of how well a compound donates protons, accepts electrons, or lowers pH in a chemical system.

94
Q

Periodic Trend: What is a binary acid? Stronger acids?

A

Binary Acid: structure=HX, can dissociate water (HX —-> H+ + X-)
Stronger Acids: Result in X- anions that are likely to separate from H+ because they are stable once they do.

95
Q

Periodic Trend: What is the periodic trend for Acidity?

A

left to right: increases, due to the electronegativity increasing, the acidity increases because the electronegative the anion is, the more acidity is has because it is more stable.
(vertical) down a group: increases, due to the increase in size of the atom because acidity also depends on the size of an anion, meaning the greater the size, the more negative charge can be delocalized and stabilized thus the increase in acidity.

96
Q

Of the following, which is the strongest acid?

A. H2O
B. H2S
C. HCl
D. HBr

A

Look at the anions (the second elements listed in the compound) and compare electronegativity and atomic radius.
Cl is more electronegative than H2S, so B is eliminated.
Br is bigger in atomic radius than both O and Cl, so the answer is D. HBr