chemistry ch. 5 test review flashcards

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the product of the frequency and wavelength equals

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1

the product of the frequency and wavelength equals

speed of the wave

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2

because C, the speed of electromagnetic radiation, is a constant, the wavelength of the radiation is

inversely proportional to wavelength

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3

according to the photo electric effect, certain kinds of light cannot eject electrons from metals due to the energy of light being too low

true

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4

if electromagntic radiation A has a lower frequency then electromagnetic radiation b, then compared to b wavelength a is

longer

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5

distance between two sucessive peaks in waves

wavelngth

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6

quantum of electromagnetic energy is

photon

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7

energy of photon is related to its

frequency

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8

the emission of electrons from metals that have absorbed photons is called

photoelectric effect

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9

a line spectrum is produced when an electron moves from one energy level to another

to a lower energy level (thing weird shaped ladder)

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10

for an electron in an atom to change from the ground state to an excited state

energy must be absorbed

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11

where do electrons circle the nucleus

in speicific allowed orbitals

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12

emitting energy

go down energy levels (e.g 4 to 1)

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13

absorbing energy

go up energy levels (e.g 2 to 3)

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14

the electron in a hydrogen atom has its lowest total energy when the electron is in its

ground state

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15

french scientist louis broglie theorized that

electrons could have a dual wave particle nature

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16

three dimensional region around a nucleus where an electron may be found is called an electron path

false

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17

according to the quantum theory of an atom, in an orbital

an electrons position cannot be known exaclty (think the rat and flashlight anaology)

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18

main energy levels of an atom are indicated by the

principal quantum theory

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19

number of sublevels within each energy level of an atom is equal to the value of

principal quantum theory

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20

an electron for which n=4 has more energy than an electron that has n=2

true

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21

the spin quantum number indicates that the number of possible spin states for an electron is an orbital is

2

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22

the set of orbtil that are speherical shaped are directed along the x,y,and z axes are called

s orbitals

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23

the major differences between a 1s orbital and a 2s orbital is that

the 2s orbital is at a higher energy level

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24

the p orbital shape

dumbell

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25

for s sublevel, number of orbital is

7

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26

how many electrons can occupy the p orbital at each energy level

6 if they have opposite spins

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27

if n is the principal quantum number of the main energy level, the max number of electrons of that energy level is

2n^2

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28

how many electrons are needed to completly fill the fourth energy level

2n^2=2(4)^2=32

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29

at n=1 the total number of electrons that can be found

2

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30

the main energy level that can hold only two electrons is the

first

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31

which of the following rules requires that each o the p orbitals at a paticular energy level recieve one electron before any of them can have two electrons

hunds rule

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32

two electrons in the 1s orbital must have different spin quantum numbrs to satisfy

the pauli's exclusion principle

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33

the sequence in which enregy sublevels are filled is specified by

the aufbau principle (bottom-top)

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34

the aufbau principle states that an electron

occupies the lowest available energy level

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35

what is the electron configuration for nitrogen atomic number 7

1s^22s^22p^3

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36

the electron for aluminum atomic number 13 is

1s^22s^22p^63s^23p^1

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37

according to bohr electrons cannot reside

in-between orbitals

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38

with a wavelegnth of 170 nm what is the frequency in hertz of this particular wavelength of uv light

c=(wavelength)(v)=1.76x10^-14 hz

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39

the electron configuration for nitrogen is 1s^22s^22p^3 what does the 3 in 2p^3 mean

electron

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40

what is the relationship between wavelength and frequency

inversely proportional

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