Chemistry Chapter 5 and 13 review
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 What was Dalton's atomic theory?
 atoms are always in motion
 the nucleus of an atom is _____ charged and has a _____ density.
 the nucleus of an atom is positively charged and as a high density.
 Dalton theorized that atoms are indivisible and that all atoms of an element are identical. Scientists now that ______________.
 atoms are all divisible.
 The number of neutrons in the nucleus of an atom can be calculated by__________
 subtracting the number of protons from the mass number
 the sum of the protons and neutrons in an atoms equals the ________
 mass number
 all atoms of the same element have the same________
 number of protons

is this true or false?
electrons have a mass of 1 amu  false
 an atom of an element with atomic number 48 and mass number 120 contains how many protons, electrons, and neutrons?
 48 protons, 48 electrons, and 72 neutrons
 how do the isotopes hydrogen2 and hydrogen3 differ?
 hydrogen3 has 2 neutrons
 the number 80 in the name bromine80 represents _____
 the mass number

is this true or false?
atoms of isotopes of an elements have different numbers of protons  false
 the periodic law states that _________________
 when the elements are arranged in order of increasing atomic number, there is a periodic repetition of their physical and chemical properties
 relative atomic masses are measured in _______
 amus

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.  65.39
 What was Bohr's contribution to the development of atomic structure?
 He proposed that electrons travel in circular orbits around the nucleus.
 What is the total number of orbitals in the third principle energy level?
 9
 what is the maximum # of electrons allowed in the 3rd energy level?
 18
 what is the maximum # of electrons that can occupy 1 orbital?
 2
 the electron configuration for fluorine is _______
 1s^2 2s^2 2p^6 3s^2 3p^1
 the 1st 3 electrons that enter into p orbitals must have _______ spins
 parallel
 the atom whose electron configuration is 1s^2 2s^2 2p^6 3s^2 3p^1 is ______
 Al
 The configuration for the outermost energy level in Ca is ______
 4s^2
 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 ____
 Cl
 the frequency and wavelength of all waves are _______
 inversely related
 The SI unit of cycles per second is called a _____
 hertz

do the following groups of atoms have the same outer configurations?
N, P, As, Bi  yes
 find the wavelength of light w/ a frequency of 2.5 X 10^13 s^ 1
 1.20 X 10^ 5
 Once the electron in a hydrogen atom absorbs a quantum of energy it:
 now in an excited state

find config. for
a.) Mg
b.) P
c.) Br
d.) Xe 
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 
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 
a.) sulfur
b.) Neon?
c.) Scandium
d.) Bromine?
e.) Strontium
f.) phosperous
g.) need to find out
h.) francium  What is the frequency of readiation whose wavelength is 6.25 X 10 ^ 5 cm?
 need to figure out
 What is the energy level of a photon whose frequency is 5.2 X 10 ^15 s^ 1?
 need to figure out
 What is the electron configuration and noble gas configuration of Phosphorus (P)?

1s^2 2s^2 2p^6 3s^2 3p^3
[Ne} 3s^2 3p^3  What is the electron configuration and noble gas configuration of Chromium (Cr)?

1s^2 2s^2 2p^6 3s^2 3p^6 4s^1 3d^5
[Ar] 4s^1 3d^5 
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 
a.) 1
b.) 2
c.) 3
d.) 4
e.) 5
f.) 6 
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 
a.) 1
b.) 1
c.) 5
d.) 7
e.) 1
f.) 3
g.) 16
h.) 5 
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 
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 
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  need to figure out
 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?
 6.00 x 10^6 cm; ultraviolet
 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?
 4.48 x 10^14 s^1; red light
 What is the energy of a photon whose frequency is 2.22 x 10^14 s^1?
 1.47 x 10^19 J
 What is the frequency of a photon whose energy is 6.00 x 10^15J?
 9.45 x 10^18 s^1

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 
d
e
a
c
f
b  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?
 1.88 x 10^2 m
 Write out the electron configurations for (a) potassium and (b) cobalt. How many unpaired electrons does each possess?
 a.) K: 1s^2 2s^2 2p^6 3s^2 3p^6 4s^1 ; K: [Ar] 4s^1; 1 unpaired electron
 Which element has the following electron configuration: 1s^2 2s^2 2p^3?
 Nitrogen (N)
 Write out the electron configurations for (a) silicon and (b) lithium. How many unpaired electrons does each possess?
 a.) Si: 1s^2 2s^2 2p^6 3s^2 3p^2 ; Si: [Ne] 3s^2 3p^2 ; 2 unpaired electrons
 Which element has the following electron configuration: 1s^2 2s^2 2p^6 3s^2 3p^3?
 Phosphorus (P)
 Write out the electron configurations for (a) iridium and (b) selenium. How many unpaired electrons does each possess?
 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
 Which element has the following electron configuration: 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^1?
 Scandium (Sc)
 What is the wavelength of a light with the frequency of 1.81 x 10 ^14 Hz?
 1.66 x 10^6 m
 What is the frequency of a light with the wavelength of 680nm?
 4.41 x 10^14 s^1
 Calculate the energy of a quantum of radiant energy, whose frequency is 3.82 x 10^14 Hz
 2.53 x 10^19 J
 What is the energy of light with the wavelength 1230nm?
 1.62 x 10^19 J
 According to the formula c= landa x new, as frequency gets larger (higher) the wavelength gets ______
 smaller
 What are rhe 4 points of John Dalton's theory?

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 wholenumber ratios to form compounds.
d.) Atoms of each element are never changed in a chemical reaction. 
Subatomic particleselectron
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 th 
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 
Protons
What did E. Goldstein find?  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

Neutron
a.) who discovered the neutron
b.) what is their mass equal to? 
a.) James Chadwick
b.) mass = to protons mass