MIDTERMS (but like look at the other decks too)

Question 1

What wavelength causes vibration?

Answer 1

infrared radiation

Question 2

What wavelength causes rotation?

Answer 2

microwave radiation

Question 3

What wavelength causes electrons to transition/be ejected?

Answer 3

UV

Question 4

Electrons in orbitals must be opposite spins

Answer 4

Pauli Exclusion Principle

Question 5

Fill orbitals half way until all in subshell are filled before filling orbitals fully

Answer 5

Hund’s rule

Question 6

Fill orbitals and subshells of lowest energy first

Answer 6

Aufbau Principle

Question 7

Aufbau Principle exceptions and why:

Answer 7

Cu and Ag, taking an electron from an s subshell to finish the d subshell and have stability, and Cr and Mo take electrons from s subshell to be half-filled stable

Question 8

Heisenberg Uncertainty Principle

Answer 8

Determining the speed or position of an electron/photon is impossible, responsible for “probabilities of distribution”/electron clouds instead of exact electron positions and speeds. Closer you get to precise location the less precise the speed is and vise versa

Question 9

Dmitri Mendeleev

Answer 9

Ordered elements from increasing atomic mass, w/elements of similar properties in the same column (he was wrong)

Question 10

stupid

Mosley

Answer 10

Ordered elements by atomic numbers (he was right)

Question 11

Why do different elements emit different spectra?

Answer 11

Because each element has a different electron configuration, thus energy levels, and therefore energy (in wavelength/frequency of photons ejected)

Question 12

Coulomb’s law

Answer 12

F=k((Q1 x Q2)/r^2)
Describes atomic radius size as a function of forces of attraction and repulsion between the nucleus and electrons and electrons and electrons, (shielding and different sized outer oribts of elements given same energy levels)

Question 13

Electronegativity trend (give directions ex. left and down)

Answer 13

Right and up

Question 14

Atomic size trend (give directions (ex. left and down are larger))

Answer 14

Left and down are larger

Question 15

Does effective nuclear charge change as it moves down a group? Why?

Answer 15

No, as the same amount of valence electrons exist for each atom down a group. ( weirdly, as the electrons are still further away, down a group decreases electron affinity/binding energy even though the effective nuclear charge is technically the same (text for clarification if this is too confusing))

Question 16

Order for determining an elements atomic size

Answer 16

1. Energy level
   a. Whether or not there are the same amount of full electron “shields”
2. Amount of protons
   a. And effective nuclear charge acting on valence electrons
3. Amount of valence electrons
   a. Electrons repel, protons in nucleus are less effective and attraction is more spread out thus making it bigger
   4.

Question 17

Metals are more prone to ______ electrons, whereas nonmetals usually _____ electrons. (gain, lose)

Answer 17

1. lose
2. gain

Question 18

Cations are _____ than their original element, whereas anions are _____. Additionally, when a cation and anion are isoelectronic, the cation is substantially smaller. Why is this? (larger, smaller)

Answer 18

1. smaller
2. larger
   because cations lose and electron, therefore decreasing electron-electron repulsion, whereas anions gain an electron, having the opposite effect. When isoelectronic, the cation has a much higher Zeff value (effective nuclear charge), increasing attraction and decreasing distance by Coulomb’s law.

Question 19

Define isoelectronic

Answer 19

Having the same number of electrons (though often not protons)

Question 20

In what direction does electron affinity increase? (ex. top left to bottom right)

Answer 20

up and to the right

Question 21

Electronegativity

Answer 21

The tendency to pull on an electron in a bond

Question 22

What changes going right on the periodic table? What changes moving down?

Answer 22

Effective nuclear charge increases right, energy level and thus shielding increases down

Question 23

Where do metallic and nonmetallic character increase/decrease?

Answer 23

Metallic character increases inversely to nonmetallic character down and left

Question 24

Name the Fundamental SI units (relevant to what we’ve learned so far) (possibly unnecessary but included just to be safe)

Answer 24

Kg, meter, second, kelvin, mole

Question 25

What do the prefixes mega, kilo, hecto, deka, deci, centi, milli, micro, and nano mean?

Answer 25

Mega - 1,000,000
kilo - 1,000
hecto - 100
deka - 10
deci - .1
centi - .01
milli - .001 (1 thousanth)
micro - .0000001 (1 millionth)
nano - .0000000001 (1 billionth)

Question 26

Charges of Ag, Zn, and Cd ions

Answer 26

Ag = +
Zn = 2+
Cd = 2+