LightPeriodic Trends

Quantum Numbers

Electron Configurati

onMixed Bag

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Mixed Bag

Which element has the electron

configuration 1s22s22p63s23p3?

If you add up the exponents,

there are 15 electrons which corresponds to phosphorous.

What is the difference

between the ground state

and the excited state for an electron?

The ground state is the lowest energy level for an electron; the excited

state is when an electron is at an energy level above its normal

state (the excited state is temporary).

How many valence electrons does

carbon have in it’s outer shell?

(Hint: first write out the e-

configuration)

C = 1s22s22p2

The second energy level is the outside shell in this case.

There are 4 electrons in the

second energy level (valence shell) for

carbon.

How many unpaired

electrons does germanium have

in it’s valence shell?

(Hint: draw the orbital diagram

first!)

After drawing the orbital diagram,

there are 2 unpaired electrons

in the germanium atom.

How many unpaired electrons

are in there in a bromine atom? How does this relate to the charge on a

bromide ion?

Bromine has 1 unpaired electron in it’s orbital diagram which makes sense since bromide

ions have a charge of -1 (they have gained 1 e-

to complete their valence shell).

Periodic Trends

Which atom would have the

largest ionization energy –Mg or Cl?

Chlorine would have the largest I.E. because it is

farther right on the periodic table

(e- are held closer so it will be harder

to rip the e- off)

Define the term “electron

affinity”

The energy involved when an

atom gains an electron.

(The opposite of ionization energy)

Rank the following

elements in order of

increasing atomic radius:

In, Al, B, Ga

B < Al < Ga < In

Rank the elements in

order of increasing metallic

character:N, Zr, Cs, Co

N < Co < Zr < Cs

Describe the comparative

size of a cation compared to the atom from which

it forms.

Cations are smaller than the atoms from which they form due

to the increasing proton/electron

attraction due to the loss of electrons.

Electron Configurati

on

What is the electron

configuration for cobalt?

Co = 1s22s22p63s23p64s2

3d7

What is the noble gas

configuration for zirconium?

Zr =[Kr]5s24d2

What is the orbital

configuration for sulfur?

1s 2s 2p

3s 3p

What do the coefficient, letter,

and exponent signify when

writing electron configurations?

Coefficient = principal energy

level

Letter = sublevel

Exponent = # of electrons in sublevel

What is the electron

configuration for iridium?

Ir = 1s22s22p63s23p64s23

d10

4p65s24d105p66s24f14

5d7

Quantum #’s

What is the maximum number of

electrons that can be contained in an:

s sublevel?p sublevel?d sublevel?f sublevel?

s sublevel – 2 e-

p sublevel – 6 e-

d sublevel – 10 e-

f sublevel – 14 e-

Which sublevels (s, p, d, or f) are

located in the fourth principal energy level?

The third energy level has s, p, d, and f sublevels

present.

How many total electrons can fit into

the third principal energy level? (Take

into account all sublevels present in the 3rd energy level)

The third energy level contains s,

p, and d sublevels so 2 +

6 + 10 = 18 total

electrons!

How do you draw arrows in an

orbital diagram and why are they drawn that way?

Arrows are drawn with the first pointing

up and the second pointing down due to the Pauli Exclusion Principal (electrons must have opposite spins in the same

orbital).

Define the Aufbau Principle and how it

relates to the electrons in an

atom.

The Aufbau Principle says that electrons completely fill from the lowest energy

level to the highest energy level.

Light

Describe the dual nature of

light

Light behaves as both a particle

and a wave.

What is the wavelength of a portion of light

having a frequency of

4.73 x 1012 Hz?

Use c = λν…

λ = 6.34 x 10-5 m

Calculate the energy of a

photon of light having a

frequency of 3.11 x 1013 kHz.

Use E = hv…

E = 2.06 x 10-17

J

What is the wavelength of a portion of light

having an energy of 1.44 x 10-12

J?

Use both light equations!

First calculate the frequency…

v = 2.17 x 1021 Hz

Then use v to find λ…

λ = 1.38 x 10-13 m

Describe why you saw colors in the flame during the

flame test lab (think about what is going

on with the electrons)

As the element samples are placed in the flame, the

electrons are given energy so they jump from the

ground state to the excited state. When the electrons

go back down to the ground state, they emit this extra

energy which we see as light (the color depends on the λ

and v.

Final JeopardyFinal Jeopardy

What are the general shapes of the four orbitals

(s, p, d, and f)?

Final JeopardyFinal Jeopardy

s = spherical

p = peanut

d = dumbell (clover)

f = flower