Chemistry Chapter 5 And 13 Review

Front 1

What was Dalton's atomic theory?

Back 1

atoms are always in motion

Front 2

the nucleus of an atom is _____ charged and has a _____ density.

Back 2

the nucleus of an atom is positively charged and as a high density.

Front 3

Dalton theorized that atoms are indivisible and that all atoms of an element are identical. Scientists now that ______________.

Back 3

atoms are all divisible.

Front 4

The number of neutrons in the nucleus of an atom can be calculated by__________

Back 4

subtracting the number of protons from the mass number

Front 5

the sum of the protons and neutrons in an atoms equals the ________

Back 5

mass number

Front 6

all atoms of the same element have the same________

Back 6

number of protons

Front 7

is this true or false?

electrons have a mass of 1 amu

Back 7

false

Front 8

an atom of an element with atomic number 48 and mass number 120 contains how many protons, electrons, and neutrons?

Back 8

48 protons, 48 electrons, and 72 neutrons

Front 9

how do the isotopes hydrogen-2 and hydrogen-3 differ?

Back 9

hydrogen-3 has 2 neutrons

Front 10

the number 80 in the name bromine-80 represents _____

Back 10

the mass number

Front 11

is this true or false?

atoms of isotopes of an elements have different numbers of protons

Back 11

false

Front 12

the periodic law states that _________________

Back 12

when the elements are arranged in order of increasing atomic number, there is a periodic repetition of their physical and chemical properties

Front 13

relative atomic masses are measured in _______

Back 13

amus

Front 14

there are 5 naturally occuring isotopes of the element zinc. the relative abundance and mass of each are as follows:

64/30 Zn = 48.89%, 63.929 amu
66/30 Zn = 27.81%, 65.926 amu
67/30 Zn = 4.11%, 66.927 amu
68/30 Zn = 18.57%, 67.925 amu
70/30 Zn = 0.62%, 69.925 amu

Calculate the average atomic madd of zinc.

Back 14

65.39

Front 15

What was Bohr's contribution to the development of atomic structure?

Back 15

He proposed that electrons travel in circular orbits around the nucleus.

Front 16

What is the total number of orbitals in the third principle energy level?

Back 16

9

Front 17

what is the maximum # of electrons allowed in the 3rd energy level?

Back 17

18

Front 18

what is the maximum # of electrons that can occupy 1 orbital?

Back 18

2

Front 19

the electron configuration for fluorine is _______

Back 19

1s^2 2s^2 2p^6 3s^2 3p^1

Front 20

the 1st 3 electrons that enter into p orbitals must have _______ spins

Back 20

parallel

Front 21

the atom whose electron configuration is 1s^2 2s^2 2p^6 3s^2 3p^1 is ______

Back 21

Al

Front 22

The configuration for the outermost energy level in Ca is ______

Back 22

4s^2

Front 23

the element having the same s and p configurations for principle energy level 3 as the element F has for its principle energy level 2 is ____

Back 23

Cl

Front 24

the frequency and wavelength of all waves are _______

Back 24

inversely related

Front 25

The SI unit of cycles per second is called a _____

Back 25

hertz

Front 26

do the following groups of atoms have the same outer configurations?

N, P, As, Bi

Back 26

yes

Front 27

find the wavelength of light w/ a frequency of 2.5 X 10^13 s^ -1

Back 27

1.20 X 10^ -5

Front 28

Once the electron in a hydrogen atom absorbs a quantum of energy it:

Back 28

now in an excited state

Front 29

find config. for
a.) Mg
b.) P
c.) Br
d.) Xe

Back 29

a.) 1s^2 2s^2 2p^6 3s^2
b.) 1s^2 2s^2 2p^6 3s^2 3p^3
c.) 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^5
d.) 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 5s^2 4d^10 5p^6

Front 30

Identify the following elements:

a.) config. = 1s^2 2s^2 2p^6 3s^2 3p^4
b.) full 2nd energy level
c.) 1st d electron
d.)7 electron in 4th energy level
e.) 2 electrons in the fifth energy level
(f.) contains 3 unpaired electrons in its 3rd energy level
g.) % electrons in 3d orbitals
h.) has its outermost electrons in 7s^1 (

Back 30

a.) sulfur
b.) Neon?
c.) Scandium
d.) Bromine?
e.) Strontium
f.) phosperous
g.) need to find out
h.) francium

Front 31

What is the frequency of readiation whose wavelength is 6.25 X 10 ^ -5 cm?

Back 31

need to figure out

Front 32

What is the energy level of a photon whose frequency is 5.2 X 10 ^15 s^ -1?

Back 32

need to figure out

Front 33

What is the electron configuration and noble gas configuration of Phosphorus (P)?

Back 33

1s^2 2s^2 2p^6 3s^2 3p^3

[Ne} 3s^2 3p^3

Front 34

What is the electron configuration and noble gas configuration of Chromium (Cr)?

Back 34

1s^2 2s^2 2p^6 3s^2 3p^6 4s^1 3d^5

[Ar] 4s^1 3d^5

Front 35

How many sublevels are in the following principal energy levels?

a.) n=1
b.) n=2
c.) n=3
d.) n=4
e.) n=5
f.) n=6

Back 35

a.) 1
b.) 2
c.) 3
d.) 4
e.) 5
f.) 6

Front 36

How many orbitals are in the following sublevels?

a.) 1s sublevel
b.) 5s sublevel
c.) 4d sublevel
d.) 4f sublevel
e.) 7s sublevel
f.) 3p sublevel
g.) fifth principal energy level
h.) 6d sublevel

Back 36

a.) 1
b.) 1
c.) 5
d.) 7
e.) 1
f.) 3
g.) 16
h.) 5

Front 37

What are the types of sublevels and number of orbitals in the following?

a.) n=1
b.) n=2
c.) n=3
d.) n=4
e.) n=5

Back 37

a.) 1s, 1 orbital
b.) 2s, 1 orbital; 2p, 3 orbitals
c.) 3s, 1 orbital; 3p, 3 orbitals; 3d, 5 orbitals
d.) 4s, 1 orbital; 4p, 3 orbitals; 4d, 5 orbitals; 4f, 7 orbitals
e.) 5s, 1 orbital; 5p, 3 orbitals; 5d, 5 orbitals; 5f, 7 orbitals

Front 38

Write a complete electron configuration of each atom.

a.) hydrogen
b.) vanadium
c.) magnesium
d.) barium
e.) bromine
f.) sulfur
g.) krypton
h.) arsenic
i.) radon

Back 38

need to figure out

Front 39

What is the wavelength of the radiation whose frequency is 5.00 x 10^15 s^-1? In what region of the electromagnetic spectrum is this radiation?

Back 39

6.00 x 10^-6 cm; ultraviolet

Front 40

An inexpensive laser that is available to the public emits light that has a wavelength of 670 nm. What are the color and frequency of the radiation?

Back 40

4.48 x 10^14 s^-1; red light

Front 41

What is the energy of a photon whose frequency is 2.22 x 10^14 s^-1?

Back 41

1.47 x 10^-19 J

Front 42

What is the frequency of a photon whose energy is 6.00 x 10^-15J?

Back 42

9.45 x 10^18 s^-1

Front 43

Arrange the following types of electromagnetic radiation in order of increasing frequency.

a.) infrared
b.) cosmic rays
c.) visible light
d.) radio waves
e.) microwaves
f.) ultraviolet

Back 43

d
e
a
c
f
b

Front 44

Suppose that your favorite AM radio station broadcasts at a frequency of 1600 kHz. What is the wavelength in meters of the radiation from the station?

Back 44

1.88 x 10^2 m

Front 45

Write out the electron configurations for (a) potassium and (b) cobalt. How many unpaired electrons does each possess?

Back 45

a.) K: 1s^2 2s^2 2p^6 3s^2 3p^6 4s^1 ; K: [Ar] 4s^1; 1 unpaired electron

Front 46

Which element has the following electron configuration: 1s^2 2s^2 2p^3?

Back 46

Nitrogen (N)

Front 47

Write out the electron configurations for (a) silicon and (b) lithium. How many unpaired electrons does each possess?

Back 47

a.) Si: 1s^2 2s^2 2p^6 3s^2 3p^2 ; Si: [Ne] 3s^2 3p^2 ; 2 unpaired electrons

Front 48

Which element has the following electron configuration: 1s^2 2s^2 2p^6 3s^2 3p^3?

Back 48

Phosphorus (P)

Front 49

Write out the electron configurations for (a) iridium and (b) selenium. How many unpaired electrons does each possess?

Back 49

b.) Se: 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^4; [Ar] 4s^2 3d^10 4p^4 ; 0 unpaired electrons

Front 50

Which element has the following electron configuration: 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^1?

Back 50

Scandium (Sc)

Front 51

What is the wavelength of a light with the frequency of 1.81 x 10 ^14 Hz?

Back 51

1.66 x 10^-6 m

Front 52

What is the frequency of a light with the wavelength of 680nm?

Back 52

4.41 x 10^14 s^-1

Front 53

Calculate the energy of a quantum of radiant energy, whose frequency is 3.82 x 10^14 Hz

Back 53

2.53 x 10^-19 J

Front 54

What is the energy of light with the wavelength 1230nm?

Back 54

1.62 x 10^-19 J

Front 55

According to the formula c= landa x new, as frequency gets larger (higher) the wavelength gets ______

Back 55

smaller

Front 56

What are rhe 4 points of John Dalton's theory?

Back 56

a.) All elements are composed of tiny indivisible particles
b.) Atoms of the same elements are identical, but different from any other element.
c.) Atoms of different elements can physically or chemically combine in simple whole-number ratios to form compounds.
d.) Atoms of each element are never changed in a chemical reaction.

Front 57

Sub-atomic particles-electron

a.) what charge?
b.) who discovered it and how?
c.) from what to what do cathode rays travel?
d.) what did Thomson propose?
e.) what did Thomson and others determine?
f.) who determined the quantity of the negative charge carried by the electron?

Back 57

a.) negative
b.) Discovered and named by J.J. Thomson in 1879 who used a cathode ray tube to pass an electric current through a gas at low pressure
c.) Cathode rays travel from a cathode (-) to an anode (+)
d.) Thomson proposed that cathode rays were composed of tiny, negatively charged particles moving at high speed
e.) Thomson and others determined that an electron has a mass of 1/2000 of an H atom
f.) Robert Milliken

Front 58

Protons

What did E. Goldstein find?

Back 58

found that some rays in a cathode tube travel in the opposite direction of a cathode ray - he named these canal rays, and realized they were composed of positively charged particles

Front 59

Neutron

a.) who discovered the neutron
b.) what is their mass equal to?

Back 59

a.) James Chadwick
b.) mass = to protons mass