Studying/ Spectroscopy

Question 1

Spectroscopy

Answer 1

study of the interaction between light and matter

Question 2

Electromagnetic Radiation

Answer 2

an oscillating electromagnetic field that propagates (travels) through space

Electric Field= up and down
Magnetic= horizontal

Question 3

Frequency

Answer 3

The number of waves passing through a single point per unit of time (usually seconds)

v= frequency
speed of light= c
unit= 1/s

Question 4

The Electromagnetic Spectrum

Answer 4

Radio, Microwave, Infrared, Ultraviolet, X-Ray and Gamma Ray

Radio- Red
Microwave- Orange
Infrared- Yellow
UV: Green
X Ray: Blue
Gamma- Purple

Question 5

What is the relationship between frequency and wavelength?

Answer 5

Inversely related

Question 6

Relationship of energy and frequency?

Answer 6

Directly proportional

Question 7

Relationship between energy and wavelength

Answer 7

inversely

Question 8

Energy of one photon…

Answer 8

is always less than one joule

Question 9

Isoelectronic

Answer 9

atoms, ions, or molecules that have the same electronic structure
and the same number of valence electrons.

Ions have elements that they are isoelectronic to

Question 10

Cation Rules

Answer 10

If in the s+p blocks (main group) then remove electrons as you would expect. Ex. 3p5 - 3p4

If in the d+f blocks remove electron from the highest n value then the highest L.

Ex. 4s2 3d6
4s 3d6
3d6

Question 11

Ionic

Answer 11

Metal-Metal
- electrons are transferred
- lattice (The lattice is formed because the ions attract each other and form a regular pattern with oppositely charged ions next to each other)

Question 12

Covalent

Answer 12

Nonmental+ Nonmental

-electrons shared
-molecule

Question 13

Metallic

Answer 13

Metal+ Metal
- sea of delocalized electrons

Question 14

Atomic Radius

Answer 14

Z eff- effective nuclear charge and since more electrons are being added to the valence shell. The nuclear charge will be greater than the shielding electrons

Question 15

Ionic Radius

Answer 15

All cations loose an electron so their nucleus pulls the electrons in making it smaller. All anions have an extra electron so the force is pulled out making the atom larger.

Question 16

Ionization Energy

Answer 16

The amount of energy needed to remove a valence electron from a gaseous ion to produce a gaseous anion. Gaseous from because electrons are more spread apart and easier to get rid of. As effective nuclear charge increases, the atomic radius decreases and makes it harder for the valence electrons to be removed. Ionization energy is inversely related to atomic radius.

Question 17

Exception to Ionization Energy

Answer 17

1. S and P block exceptions. In the P block the electrons have a higher energy and they are further away from the nucleus than the S block. This means that they are easier to remove. So in cases such as Beryllium and Boron, Boron will have less ionization energy since it is in the P block.
2. N and O and P and S. In these cases the P block as 3 orbitals and cases where the orbital has two electrons, they will repel each other making it have less ionization energy. So O and S have less ionization energy.

Question 18

Second and Third Ionization energy

Answer 18

The second energy and third will always be much greater than the first because it is harder to remove an electron from a positively charged species. Cation

Question 19

What are periodic trends

Answer 19

1. Atomic Radius
2. Ionic Radius
3. Ionization Energy

Question 20

L value 0

Answer 20

s
shape: sphere

Question 21

L value 1

Answer 21

p
shape: node

Question 22

Binary Ionic

Answer 22

Metal + Nonmetal
[ide]

Question 23

Charge of Al

Answer 23

+3

Question 24

Charge of Zn

Answer 24

+2

Question 25

Charge of Ag

Answer 25

+1

Question 26

Acetate

Answer 26

C2H3O2 -

Question 27

Hydroxide

Answer 27

OH-

Question 28

Cyanide

Answer 28

CN-

Question 29

Peroxide

Answer 29

O2 2-

Question 30

Oxide

Answer 30

O2-

Question 31

Ammonium

Answer 31

NH4 +

Question 32

Ammonia

Answer 32

NH3

Question 33

Carbonate

Answer 33

CO3 2-

Question 34

phosphate

Answer 34

PO4 3-

Question 35

sulfate

Answer 35

SO4 2-

Question 36

chlorate

Answer 36

ClO3 -

Question 37

nitrate

Answer 37

NO3 -

Question 38

Principle quantum letter

Answer 38

n describes the overall energy and size of the electron

Question 39

quantum letter l

Answer 39

angular momentum describes the shape of the orbital

Question 40

quantum letter ml

Answer 40

magnetic orbitals orientation in space amount of orbitals

Question 41

Binary Acids

Answer 41

Hydrogen with a singular nonmetal hydro- [ic] acid ex. HF- hydrofluoric acid

Question 42

Oxyacid

Answer 42

acids with oxyanions if it ends in "ate" then [ic] if it end in 'ite' then [ous]

Question 43

empirical formula

Answer 43

a chemical formula that can represent a RELATIVE number of each element in a molecule

Question 44

molecular formula

Answer 44

a chemical formula that represents the EXACT/ACTUAL number of each element in a molecule

Question 45

determining the empirical formula

Answer 45

1st. Find the moles of each element 2. Then divide by the smallest subscript

Question 46

determining the molecular formula

Answer 46

1. Given the molar mass of the molecular formula 2. Find the mm of the empirical formula mm (molecular)/ mm (emp)

Question 47

combustion analysis/ reaction

Answer 47

An organic molecule made of hydrocarbons + O2 will combust to make H2O+ CO2.

Question 48

Valence electrons

Answer 48

the outmost highest energy electrons in an atom and they participate in all bonding and chemical reactions.

Question 49

Electronegativity

Answer 49

measure of how much an atom wants an electron. F has the most electronegativity.

Question 50

The Pauli exclusion principle

Answer 50

states that no two electrons in a given atom can share the same set of four quantum numbers

Question 51

HCN

Answer 51

hydrocyanic acid

Question 52

HC₂H₃O₂

Answer 52

acetic acid