Exam 3 Review

Question 1

Electromagnetic Radiation

Answer 1

type of energy described by a wave composed of oscillating electric and magnetic field

Question 2

Speed of light in vacuum (c)

Answer 2

3x10^8 m/s

Question 3

frequency (curvy v)

Answer 3

number of wave crests or cycles that travel through a stationary point in a given amount of time (measured in cycle per second, s^-1, or Hz)

Question 4

Velocity (flat v)

Answer 4

flat v = (wavelength)(frequency)

Question 5

Vacuum (flat v) = speed of light (c)

Answer 5

c= (wavelength)(frequency)

Question 6

Electromagnetic Spectrum (in term of largest wavelength to shortest wavelength)

Answer 6

radio wave<microwave<infrared wave< visible light<ultraviolet wave<x-ray< gamma ray

Question 7

Interference

Answer 7

superposition of 2 or more waves overlapping in space resulting in either increase or decrease of amplitude

Question 8

Constructive Interference

Answer 8

2 waves overlap with each other making a new higher frequency wave

Question 9

Destructive Frequency

Answer 9

2 waves (where the crest aligns with the trough) lowering the amplitude

Question 10

photon

Answer 10

massless particle of light

Question 11

Planck’s Constant

Answer 11

h = 6.626x10^-34 Js

Question 12

Ephoton

Answer 12

= (hc)/(wavelength)

Question 13

En (energy associated with each level in a H atom)

Answer 13

En = (-2.18x10^-18J)/(n^2)

Question 14

Change in energy between 2 levels in H atom

Answer 14

Delta H - E final- E initial

-2.18x10^-18(1/nf^2-1/ni^2)

Question 15

delta E > 0

Answer 15

a photon is absorbed to excite the electron to higher level (absorb energy)

Question 16

delta E < 0

Answer 16

a photon is released and electron relaxes to lower energy level (release energy)

Question 17

Orbital

Answer 17

represents a probability distribution map that shows where an electron is likely located

Question 18

principle quantum number

Answer 18

n –> principle shell/level, general region of electron

Question 19

angular momentum quantum number

Answer 19

l –> subshell, shape of the orbital

Question 20

magnetic momentum quantum numbers

Answer 20

Ml (2(l) + 1) –> orientation of the orbital

Question 21

spin quantum number

Answer 21

ms (-1/2, 1/2) –> direction of “spinning” electron

Question 22

phase

Answer 22

the sign of the amplitude of a wave (positive or negative)

Question 23

spin quantum number (Ms)

Answer 23

a half-integer value that denotes the “spin” of the electron (-1/2,1/2)

Question 24

Orbital Diagram

Answer 24

symbolizes electron as arrows and the orbital as a line or a box

Question 25

Pauli Exclusion Principle

Answer 25

no 2 electrons is an atom cannot have the same set of four quantum number -the arrows go in the different directions in the same box

Question 26

Shileding

Answer 26

the effect of an electron of repulsion by electrons in lower energy will shield it from the full effects of nuclear charge

Question 27

Effective Nuclear Charge (Z eff)

Answer 27

actual nuclear charge that is experienced by the electron

Question 28

Aufoam Principle

Answer 28

electrons fill lower energy orbitals first before filling higher orbitals needs to fill up 1s^2 2s^2 then 2p^1

Question 29

valence electrons

Answer 29

the electrons in the outermost shell

Question 30

core electrons

Answer 30

all other elements not in the outermost shell

Question 31

paramagnetic

Answer 31

the state of an atom or ion that contains unpaired electrons (they are attracted to an external magnetic field)

Question 32

diamagnetic

Answer 32

the state of an atom or ion that contains all electrons are paired (they are not attracted to an external magnetic field)

Question 33

Atomic Radius

Answer 33

increases going down and decreases going from left to right

Question 34

Cations

Answer 34

much smaller than their neutral atom counterpart

Question 35

Anions

Answer 35

much larger than their neutral atom counterpart

Question 36

Isoelectronic

Answer 36

atoms or ions that have the same EC

Question 37

Metallic Charges

Answer 37

increases top to bottom and decreases from left to right

Question 38

ionization energy

Answer 38

the energy required to remove electron from an atom or ion in the gaseous state (decreases top to bottom and increases left to right)

Question 39

Electron Affinity

Answer 39

the energy change associated with the gaining of an electron by an atom or anion in a gaseous state (decreases top to bottom and increases left to right)

Question 40

Octet Rule

Answer 40

the tendency of atoms of most main-group elements to posses or share 8 electrons in their outermost shell to obtain a stable EC (that of the nearest noble gas) EXCEPT for H, He, Li ( they follow duet rule)

Question 41

Electronegativity

Answer 41

refers to the ability of an atom to attract electrons toward itself in a chemical bond

Question 42

Resonance Structure

Answer 42

lewis structure of a molecule or polyatomic ion that differ only int he position of their electrons

Question 43

Bond Order Formula

Answer 43

(number of bonds around central atoms)/(number of terminal atoms)

Question 44

formal charge

Answer 44

the charge an atom would have if all bonding electrons are shared equally between other atoms

Question 45

FC Formula

Answer 45

(number of valence electrons)- 1/2(number of bonding electrons)-(number of non bonding electrons)

Question 46

Properties of ionic compounds

Answer 46

-solid at room temperature -high mp and bp -good conductor of electricity when dissolved in water

Question 47

Properties of molecular compounds

Answer 47

-liquid or gas at room temperature -low mp and bp -poor conductor of electricity when dissolved in water

Question 48

Hund's Rule

Answer 48

every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied -all the arrows are fulled up in the boxes first before the down arrows occur