Exam 2 Review

Question 1

what is wavelength

Answer 1

lamba, distance between two peaks of a wave

Question 2

what is frequency

Answer 2

v, the number of wave cycles per second

Question 3

what is amplitude

Answer 3

a, the height

Question 4

what is the electromagnetic spectrum

Answer 4

the full range of electromagnetic radiation, organized by frequency or wavelength

Question 5

constructive vs destructive interference

Answer 5

constructive two waves overlap to combine to create a larger wave, destructive two waves overlap and cancel each other out

Question 6

what is a node

Answer 6

one or more points between the two ends of a wave that are not in motion, probability of finding a electron is zero, amplitude is 0

Question 7

explain quantization

Answer 7

energy levels within an atom or molecules can only exist at specific real values, n

Question 8

what is the photoelectric effect

Answer 8

light causes electrons to be ejected from a metal surface, shows that light can act like particles, photons

Question 9

explain line spectra

Answer 9

when atoms are excited, their electrons jump to higher energy levels, and when they fall back down emit light at a specific wave length, rydberg equation

Question 10

explain bohr’s model

Answer 10

electrons are found in orbits around the nucleus, orbits farther apart are higher in energy

Question 11

explain absorption

Answer 11

atom absorbs energy around it causing an electors to jump to a higher level, ∆E is positive

Question 12

explain emission

Answer 12

atom releases energy causing electron to move to a lower energy level, ∆E is negative

Question 13

what does the Heisenberg uncertainty principle state?

Answer 13

we cant exactly know where an electron in, but we can predict regions where it is most likely to be found

Question 14

what does the quantum number n stand for

Answer 14

size/ energy level

Question 15

what does the quantum number l stand for

Answer 15

shape, 0 to n-1, spdf

Question 16

what does the quantum number ml stand for

Answer 16

orientation, from 1 to -1

Question 17

what does the quantum number ms stand for

Answer 17

spin, +1/2 or -1/2

Question 18

how many lobes does the p orbital have

Answer 18

2

Question 19

how many lobes does the s orbital have

Answer 19

1

Question 20

how many lobes does the d orbital have

Answer 20

4

Question 21

how many lobes does the f orbital have

Answer 21

6 or 8

Question 22

what is the Pauli exclusion principle

Answer 22

np two electors can have the exact set of 4 quantum numbers

Question 23

valence vs core electrons

Answer 23

valence are the outermost electrons, highest energy level, core are inner.

Question 24

ground vs excited state

Answer 24

ground will have all shells full, excited will have one not full

Question 25

what is zeff

Answer 25

amount of positive charge an electron feels, z-s, # protons - inner shell electrons

Question 26

what is ionization energy

Answer 26

amount of energy required to remove an electron in the gas phase

Question 27

what is covalent radius

Answer 27

1/2 the distance between nuclei

Question 28

what is electron affinity

Answer 28

energy change for the process of adding an electron to an atom in the gas phase, result in a anion

Question 29

what is a ionic bond

Answer 29

electrons are transferred and ions are held together electrostatically

Question 30

what is a covalent/molecular bond

Answer 30

electrons are shared between atoms

Question 31

ionic vs covalent bonds

Answer 31

ionic has metal and non metal, covalent has two non metals

Question 32

how are electrons held together in a ionic bond

Answer 32

in a lattice structure, metal donates electrons to the non metal

Question 33

describe non polar covalent

Answer 33

shared evenly, two of same electronegativity, pure

Question 34

describe polar covalent

Answer 34

shared unevenly, two different non metals

Question 35

what is electronegativity

Answer 35

the ability of an atom in a COMPOUND to draw electrons to itself