chapter 6/7 review

Question 1

waves

Answer 1

a disturbance that transmits energy through space

Question 2

the longer the wavelength

Answer 2

the lower the frequency

Question 3

the shorter the wavelength

Answer 3

the higher the frequency

Question 4

the speed of light (c)

Answer 4

2.998x10^8 m/s

Question 5

speed=

Answer 5

frequency times wavelenth

Question 6

wavelength (λ) is measured in___
frequency (v) is measured in ___

Answer 6

λ= meters (m)
v= hertz (Hz)/ inverse seconds

Question 7

frequency (V)

Answer 7

the number of waves passing a point in a given amount of time

Question 8

EM spectrum pneunonic

Answer 8

Red Men Interview Very Ugly Xylophone Guys

Question 9

EM spectrum longest wavelength to shortest wavelength

Answer 9

radio, microwaves, infrared, visible, ultra-violet, x-rays, gamma rays

Question 10

constructive interference

Answer 10

when two like waves combine to create a larger wave

Question 11

destructive interference

Answer 11

when two unlike waves combine to create no wave (flat line)

Question 12

diffraction

Answer 12

a change in the direction of waves as they pass through an opening or around a barrier in their path

Question 13

refraction

Answer 13

bending of waves as they pass from one medium to another

Question 14

photon

Answer 14

a particle of light

Question 15

C=

Answer 15

λV

Question 16

what were the main issues of classical physics

Answer 16

experimental data did not agree with theory, had to change theory
blackbody radiation, photoelectric effect, atomic emission spectra

Question 17

blackbody radiation

Answer 17

energy like matter is discontinuous or quantized
the quantum EM radiation is proportional to the frequency of the radiation

Question 18

Energy=

Answer 18

h times V

Question 19

planks constant

Answer 19

6.626x10^-34 Js

Question 20

photoelectric effect

Answer 20

when light strikes a metal, electrons are emitted
emission only occurs at certain threshold frequencies

Question 21

atomic emission spectra

Answer 21

when an electron is struck with energy, it is excited and emits light

Question 22

bohr model of the atom

Answer 22

-electrons move around the nucleus in a set of circular orbits
-as long as an electron stays in its given orbit, not energy is emitted, with a fixed radius and energy
-an atom emits energy as a photon when the electron FALLS from to an orbit with a SMALLER radius and LOWER energy

Question 23

E (with wavelength)

Answer 23

hc/λ

Question 24

ground state

Answer 24

lowest energy level
n=1

Question 25

excited state

Answer 25

electron moves out of the ground state into a state with a HIGHER n value

Question 26

when an electron falls from an excited state to a lower energy level,

Answer 26

it emits a photon

Question 27

increasing atomic number (Z) results in

Answer 27

a greater effective charge

Question 28

λ (Broglie wavelength)=

Answer 28

h/p or h/ mass times speed/velocity

Question 29

you can never know the exact ___ and ____, you will either know one or another

Answer 29

position or momentum

Question 30

types quantum numbers

Answer 30

n= the principle quantum number l= the orbital angular momentum quantum number ml= angular momentum quantum number ms= electron spin quantum number

Question 31

n (principle quantum number) describes and accepted values

Answer 31

the shell where the electron is located n can have positive, whole-number values, non-zero ex) 1,2,3,4...

Question 32

all electrons with the same value of n are in the same

Answer 32

principle electron shell or level

Question 33

l (angular momentum) describes and its accepted values

Answer 33

describes the SHAPE of the orbital where the electron is located describes the subshell where the electron is located can have zero, and positive whole-number values ex) 0,1,2,3... it CANNOT be the same value as n, has to be at least 1 lower!!!

Question 34

subshells of l

Answer 34

l=0, s l=1, p l=2, d l=3, f

Question 35

ml (magnetic quantum number) is described and accepted values are

Answer 35

describes the orientation of the orbital where the electron is located can have negative, zero, and whole-number values from -l to +l m,=-1,0,1

Question 36

ms (spin quantum number)

Answer 36

describes the orientation of the electron spin can have +1/2 or -1/2 values only

Question 37

orbitals

Answer 37

where electrons are likely to be found around the nucleus

Question 38

the number of l values in a subshell is equal to

Answer 38

the number of allowed ml values (2l+1)

Question 39

s orbitals have a ___ shape (l=0)

Answer 39

spherical shape

Question 40

p orbitals have a ___ shape (l=1)

Answer 40

two lobes with a node where e- cannot go

Question 41

d orbitals have a ___ shape (l=2)

Answer 41

multiple lobes and nodes

Question 42

f orbitals

Answer 42

l=3

Question 43

an electron with higher principle quantum energy level will

Answer 43

generally be higher in energy

Question 44

in a single atom, subshells with the same

Answer 44

principle number are DEGENERATE

Question 45

in a multi-electron atom, sublevels with the same principle energy level are

Answer 45

no longer degenerate

Question 46

electrons close to the nucleus ____ causing them to have a LOWER____ and a HIGHER_____

Answer 46

-SHEILD electrons farther out from the nucleus -effective nuclear charge (zeff) -energy

Question 47

Pauli exclusion principle

Answer 47

no two electrons can have the same quantum numbers

Question 48

afabu principle

Answer 48

electrons fill lower energy orbitals first

Question 49

hunds rule

Answer 49

when multiple degenerate orbitals are available, electrons fill each singly before paring with parallel spins

Question 50

orbitals with the same __ and ___ are degenerate

Answer 50

n and l

Question 51

effective nuclear charge

Answer 51

increases across the periodic table due to shielding zeff= Z- S (number of protons minus number of core electrons)

Question 52

valance electrons

Answer 52

electrons in the outermost shell

Question 53

exceptions to electron configuration filling

Answer 53

chromium, molybdenum, copper, silver, and gold

Question 54

paramagnetic

Answer 54

unpaired e-

Question 55

diamagnetic

Answer 55

no unpaired e-

Question 56

ionization energy

Answer 56

the amount of energy required to remove an electron from a neutral atom in its gas phase always ENDOTHERMIC

Question 57

ionization trend plus exceptions

Answer 57

increases from the left to the righter and up the periodic table exceptions: group 2 and 13 switch and group 15 and 16 switch

Question 58

electron attachment enthalpy

Answer 58

the change when a gaseous atom adds an electron, forming a gaseous anion X(g) + e- ---> X-(g) EXOTHERMIC and negative

Question 59

electron affinity

Answer 59

energy required to detach an electron from an anion with a negative 1 charge X-(g) ---> X(g) + e- positive and ENDOTHERMIC

Question 60

electron affinity and attachment trend plus exceptions

Answer 60

increases favorability from the left to right and up the periodic table exceptions: row 2 (less favorable) and 3 switch noble gases very unfavorable groups 1 and 2 switch and groups 15 and 14 switch

Question 61

atomic radius and trend

Answer 61

measure of the size of an atom increases from the right to left and down the periodic table

Question 62

ionic radius: cations: anions:

Answer 62

cations=smaller anions= larger

Question 63

electronegativity and trend

Answer 63

measure of the ability of an atom to attract electrons to itself increases from the left to right and up the periodic table noble gases excluded francium is least EN and fluorine is most EN