Chapter 3 - Electronic Structure + Periodic Properties of Elements + wavelength/energy

Question 1

So4^-2

Answer 1

Sulfate Ion

Question 2

NH4+

Answer 2

Ammonium ion

Question 3

OH-

Answer 3

Hydroxide ion

Question 4

NO3-

Answer 4

Nitrate ion

Question 5

CO3^-2

Answer 5

Carbonate ion

Question 6

PO4^-3

Answer 6

Phosphate ion

Question 7

Prefix for one?

Answer 7

Mono

Question 8

Prefix for two?

Answer 8

Di

Question 9

Prefix for three?

Answer 9

tri

Question 10

Prefix for four?

Answer 10

tetra

Question 11

Prefix for five?

Answer 11

penta

Question 12

Prefix for six?

Answer 12

hexa

Question 13

HSO4^-1

Answer 13

hydrogen suflate/ bisulfate ion

Question 14

HCO3^-1

Answer 14

hydrogen carbonate/ bi carbonate

Question 15

H2PO4^-1

Answer 15

dihydrogen phosphate

Question 16

What are Ionic Compounds?

Answer 16

Metal + NonMetal

Question 17

What are Molecular Compounds?

Answer 17

2 or more nonmetals

Question 18

How do you name a Ionic Compound?

Answer 18

Cation (metal) + Anion (nonmetal) (ends in -ide)
EX: KCl = Potassium Chloride
- DO NOT ADD PREFIXES (thats ONLY for molecular compounds)

Question 19

How do you name a Molecular Compound?

Answer 19

Anion + prefixes (mono, di, tri, tetra, penta, or hexa)
EX: BrI3 = Bromine triiodide
- If there’s only one of the first anion, DO
NOT put mono
N2O2 = Dinitrogen tetraoxide

Question 20

How do you name a Ionic Compound with a transition metal cation?

Answer 20

1. Find the charge of the anion (the nonmetal).
   - The charge of the anion is the amount of electrons needed to reach the noble gases.
2. The charge of the anion will be the same charge for the cation (transition metal). Write this charge in the formula.
   - Remember that if there’s more than one of the cation that the charge might be different from the anion
   - EX: Cr3(PO4^-3)2
   
   • The charge of Cr is 2 instead of 3 because
     3x2 = 6, which is the same for PO4 (-3x2= 6)

Question 21

What happens when you have a negative (-) charge on an atom?

Answer 21

The atom has gained an electron

Question 22

What happens when you have a positive (+) charge on an atom?

Answer 22

There atom lost an electron

Question 23

Electron Configuration

Answer 23

1s ->2s ->2p -> 3s -> 3p -> 4s -> 3d -> 4p -> 5s -> 4d -> 5p -> 6s -> 4f -> 5d -> 6p -> 7s -> 5f -> 6d -> 7p

Question 24

How do you write an electron configuration?

Answer 24

• Follow the ortibal pattern on the periodic table
• If the element has a configuration that includes a noble gas (EX: Kr 18), then you don’t have to write the whole configuration, start with the nearest noble gas then write out the rest
  EX:
  S = [10Ne] 3s2 3p4

Question 25

How do you write an electron configuration for a cation or anion?

Answer 25

If you have a cation, electrons are lost from the "s" orbital FIRST, then d orbital If you have an anion, electrons are added to the d, p, or f orbitals depending on where the original element with no charge ends.

Question 26

What is the trend of the relative size of an atom on the periodic table?

Answer 26

the atoms get bigger as we proceed down or to the left in the periodic table - This would make francium (Fr) the biggest element on the periodic table and helium (He) the smallest element on the periodic table

Question 27

What is the size of anions and cations compared their coresponding element?

Answer 27

Anion > Element > Cation

Question 28

What is the trend of first ionization energy on the periodic table?

Answer 28

the ionization energy gets bigger as we proceed up or to the right of the periodic table - The smaller the atom the higher the first ionization energy - This means that He would have the highest ionization energy on the periodic table and Fr would have the lowest ionization energy on the periodic table.

Question 29

What is the trend of electronegativity on the periodic table?

Answer 29

Highest = Fluorine 2nd highest = Cl, O 3rd highest = Br, N, S lower values = C, H, etc - Atoms that are closest to a Noble gas electronic configuration (aka Halogens) are generally the most electronegative

Question 30

What are quantum numbers?

Answer 30

n, l, ml, ms - Each quantum number describes a different feature of the electron. (So four numbers = four features)

Question 31

What does the quantum number "n" mean?

Answer 31

- n” is the principle quantum number (they start with 1,2,3....) - Planck’s quantum energy levels that correspond to increasing “shell” distances from the nucleus

Question 32

What does quantum number "l" mean?

Answer 32

“angular momentum quantum number” - This corresponds to the “shape” of an orbital, or “orbital type - “l” cannot be negative and it cannot equal the first quantum number, “n”

Question 33

What are the different values for quantum number "l" and what do they mean?

Answer 33

There are only four different “l” values: “l” = 0 equals an “s”(spherical) orbital. “l” = 1 equals a “p” orbital (“pi-shaped”). “l” = 2 equals a “d” orbital. “l” = 3 equals an “f” orbital.

Question 34

What does quantum number "ml" mean?

Answer 34

“magnetic quantum number” An “l =0” value (“s” orbital) can only have an “ml” value equal 0 (-0 or +0 = 0 !). Therefore there is only one kind of “s” orbital. An “l” =1 value (“p” orbital) can have “ml” values of -1, 0, +1. So there are three kinds of “p” orbitals. An “l” = 2 value (“d” orbital) can have “ml” values of -2, -1, 0, +1, +2. So there are five kinds of “d” orbitals. An “l” = 3 value (“f” orbital) can have “ml” values of -3, -2, -1, 0, +1, +2, +3. So there are seven kinds of “f” orbitals.

Question 35

What does quantum number "ms" mean?

Answer 35

“ms” is the fourth quantum number and is related to the magnetic properties of an electron. It’s called “spin” It only two values here: - ½ and + ½ (usually written as +-1/2

Question 36

Where (at what quantum level) do each of these n orbitals first appear?

Answer 36

When “n” = 1, “l” can only be = “0” i.e. an “s” orbital. At level 1 we only have an “s” orbital! When “n” = 2, “l” can be either “0” or “1” i.e. an “s” orbital or “p” orbitals (one “s” orbital, three possible “p” orbitals) When “n” = 3. “l” can be either “0”, or “1” or “2” i.e. “s” or “p” or “d” orbitals- (one “s” orbital, three “p” orbitals, five possible “d” orbitals) When “n” = 4. “l” can be either “0”, or “1” or “2” or “3” i.e. “s” or “p” or “d” or “f” orbitals- (one “s” orbital, three “p” orbitals, five “d” orbitals, and seven possible “f” orbitals).

Question 37

Are all the quantum numbers equally important to understanding the underlying chemistry of that element?

Answer 37

The first two numbers are really important (and easy to follow) since they tell us what was the last orbital filled and therefore where we are in the periodic table. Examples: (4,0, x,x) = a “4s” orbital (K or Ca) (3,2,x,x) = a “3d” orbital (an element somewhere between Sc and Zn)

Question 38

What is wavelength?

Answer 38

symbol = “λ”, lambda - The distance between two peaks - Usually measured in "nm" (remember that 10^9 nm = 1 m) Equations to find wavelength: - Ephoton =hν = hc/λ or λ = hc/ ΔE - λ ν = c

Question 39

What energy level and light is Lyman series?

Answer 39

energy level = 1 light = ultraviolet (UV)

Question 40

What energy level and light is Balmer series?

Answer 40

energy level = 2 light = visible light (300nm - 700nm)

Question 41

What energy level and light is Paschen series?

Answer 41

energy level = 3 light = infrared light (IR)

Question 42

What is the equation to find energy of hydrogen?

Answer 42

E = -kZ^2/n^2 -k = rydberg's constant for hydrogen Z = atomic number n = energy level

Question 43

Equation to calculate wavelength?

Answer 43

λ = hc/ ΔE ΔE = change in energy (ΔE = Efinal - Einitial) h = planck's constant (6.626 x10^-34 (Joule x sec)/ photon ) v = frequency c = speed of light (2.998 x 10^8 m/s) λ = wavelength ( in m, NOT nm)

Question 44

How to find moles of energy?

Answer 44

Emole = Ephoton x No No = 6.022 x10^23 photons/mole

Question 45

Bohr equation?

Answer 45

∆E = E(final) –E(initial) = -R[1/n2 (final)- 1/n2 (initial)] R = 2.179 x 10^-18 J/photon