physical science chapter 8 online assessment
excited states
as applied to an atom, describes the energy state of an atom that has electron in a state above the minimum energy state for that atom; as applied to nucleus, describes the energy state of nucleus that has particles in a state above the minimum energy state for that nuclear configuration
Equal to 1/12 the mass of a carbon-12 atom, the is used to describe the relative mass of an atom.
atomic mass unit
The word.... comes from the Greek for indivisible and was used by early philosophers to describe their idea that a substance could only be divided so far before it wasn't that substance any longer.
atoms
isotope
atoms of an element with identical chemical properties but with different masses; isotopes are atoms of the same element with different numbers of neutron
Which of the following are letters associated with energy sublevels in an atom? (Select all that apply.)
d p s f
angular momentum quantum
defines energy sublevels within the main energy levels
I
energy level
En
energy of particular
E1
energy of the innermost orbit
EL
energy of the orbit closest to the nucleus
EH
energy of the orbit farthest from the nucleus
For an electrically neutral atom, the number of protons is _____ the number of electrons.
equal to
f
frequency
metals
gain electrons to form negative ions
nonmetals
gain electrons to form negative ions
O
gains 2
Br
halogen
metals
large blue area on the left
Mg
loses 2
line spectrum
narrow lines of color in an otherwise dark spectrum; these lines can be used as "fingerprints" to identify gases.
Pauli Exclusion Principle
no two electrons in an atom can have the same four quantum numbers; thus, a maximum of two electrons can occupy a given orbital
He
noble gas
Group 8A
noble gases
#
number of electrons in the given energy sublevel
Two electrons in the same orbital but spinning in opposite directions are an electron
pair
h
planck's constant
n
principal energy sublevel
n
quantum number for an orbit
Somewhat poorly named, Blank 1Blank 1 atoms, Incorrect Unavailable Blank 2Blank 2 help, Incorrect Unavailable elements are both metallic and more abundant than gold and silver.
rare earth
Figure A represents the orbitals, figure B is the orbitals, and figure C is the orbitals
s p d
nonmetals
small green area on the right
semiconductors
small yellow area resembling a staircase
Electron dot notation consists of the... of the element and one dot for each...electron in an atom of the element.
symbol outer
electron configuration
the arrangement of electrons in orbitals
ground state
the energy state of an atom with electrons at the lowest energy state possible for that atom
atomic number
the number of protons in the nucleus of an atom
magnetic quantum number
the orientation of an orbital is space
orbital
the region of space around the nucleus of an atom where an electron is likely to be found
atomic mass unit
the relative mass unit (u) of an isotope based on the standard of the carbon-12 isotope, which is defined as a mass of exactly 12.00u; one atomic mass unit (1 u) is 1/12 the mass of carbon-12 atom
mass number
the sum of number of protons and neutrons in a nucleus defines the mass number of an atom; used to identify isotopes- for example, uranium-238
atomic weight
the weight average of the masses of stable isotopes of an element as they occur in nature, based on the abundance of each isotope of the element and the atomic mass of the isotope compared to C-12
nucleus
tiny, relatively massive and positively charged center of an atom containing protons and neutrons; the small, dense center of an atom
Heisenberg uncertainty principle
you cannot measure both the exact momentum and the exact position of a subatomic particle at the same time; the more exactly one of the two is known, the less certain you are of the value of the other
de Broglie equation
λ = h/mv
The principal quantum number is given the symbol... and has positive, whole-number values starting with...
<s v="1"><p><t s="9">n</t></p></s> 1
S
1
Calculate the de Broglie wavelength of a 1.67 x 10-27 kg neutron with a velocity of 2.70 x 108 m/s. λ = hmvhmv and h = 6.63 x 10-34 J⋅s and J = kg⋅m2s2kg⋅m2s2.
1.47 x 10-15 m
An unknown element has two primary isotopes, one with a relative abundance of 99.63 percent and a mass of 14.00307 u, and another with a relative abundance of 0.37 percent and a mass of 15.0011 u. What is the atomic weight of this element?.... (Give your answer to 4 decimal places.)
14.0067
What is the frequency of the energy emitted when the electron of a hydrogen atom moves from the n = 1 to the n = 2 energy level? x 1015 Hz
2.47
The energy of a photon of light with a frequency of 4.3 x 1014 Hz is... x 10-20 J. Note: h = 6.63 x 10-34 J⋅s
2.85
P
3
Which of the following electron sublevels has the highest energ
3d
What is the wavelength of the violet line (n = 6) in the hydrogen line spectra according to Balmer's equation? ______ x 10-7 m 1λ1λ = R(122122 - 1n21n2) where R = 1.097 x 107 1/m
4.10
d
5
What is the wavelength associated with a 0.43 kg soccer ball that is kicked at a velocity of 25 m/s? λ = hmvhmv and h = 6.63 x 10-34 J⋅s and J = kg⋅m2s2kg⋅m2s2...e x 10-35 m
6.16
Planck's constant
6.626 x 10^-34
Rank the following orbitals from lowest to highest energy. Place the orbital with the lowest energy at the top of the list and the orbital with the highest energy at the bottom of the list.
6s 4f 5d 6p
f
7
proton
A subatomic particle that has a positive charge and that is found in the nucleus of an atom
Which element has the electron configuration 1s22s22p63s23p1?
Al
K
Alkali metal
Mg
Alkaline Earth Metal
What is the correct definition of atomic weight
Atomic weight is the weighted average, relative to carbon-12, of all naturally occurring isotopes for a given element.
There were a few limitations of the ______ model of the atom, including no explanation for the quantized orbits and his rule of radiationless orbits
Bohr
Which of the following statements correctly describe cathode rays? (Select all that apply.)
Cathode rays are identical no matter what their source. The discovery of cathode rays showed that an atom can be broken down into smaller particles. A cathode ray consists of negatively charged particles.
frequency and energy equation
E=hf
Which of the following statements correctly describe the atomic number of an element? (Select all that apply.)
Each element has its own unique atomic number. The atomic number is equal to the number of protons in the nucleus.
Which of the following options correctly describe electron dot notation? (Select all that apply.)
Electron dot notation represents the outer electrons in a given element. The electron dot notation will be the same for all members of the same family.
What does it mean for energy to be quantized?
Energy is absorbed or emitted in discrete units.
quanta
Fixed amounts; usually referring to fixed amounts of energy absorbed or emitted by matter. (quanta is plural, and quantum is singular)
Rank the following elements from the least number of outer electrons to the most number of outer electrons. Place the element with the least number of outer electrons at the top of the list and the one with the most at the bottom.
Fr Mg At Rn
Br
Gains 1
Group 7A
Halogens
Which of the following statements about ions is correct?
Ions can be positive or negative.
Na
Loses 1
What is the limitation of the Bohr model of the atom
The Bohr model cannot account for the behavior of multielectron species.
What does the equation based on the Bohr model of the atom (shown) allow one to calculate?
The energy that is emitted or absorbed when the hydrogen electron moves between energy states
What information is contained in the atomic number of an electrically neutral element? (Select all that apply.)
The number of electrons The number of protons
Which of the following options correctly describe the problems with the solar system model of the atom? (Select all that apply.)
The solar system model of the atom describes a situation in which the atom would collapse. Orbiting electrons would emit light. Orbiting electrons would accelerate.
Which of the following statements correctly describe the magnetic quantum number? (Select all that apply.)
This value describes the orientation of orbitals in space around the nucleus.
What is an electron pair?
Two electrons with opposite spin directions in the same orbital
neutron
a neutral subatomic particle that is found in the nucleus of an atom
electron-dot notation
a notation made by writing the chemical symbol of an element with dots around the symbol to indicate the number of outer orbital electrons
electron pair
a pair of electrons with different spin quantum numbers that may occupy an orbital
protons
a quantum of energy in a light wave; the particle associated with light
group 1A
alkali metals
Group 2A
alkaline earth metals
Rutherford's famous gold-foil experiment tracked the location of... particles impacts on a thin metal foil in order to understand the nature of radioactivity.
alpha
ion
an atom or particle that has a net charge because of the gain or loss of electrons; polyatomic ions are groups of bonded atoms that have a new charge
semiconductor
an element that has properties between those of metals and nonmetals
metal
an element that is a good conductor of electricity, has a shiny surface, is malleable and ductile
nonmetal
an element that is generally a gas or a dull brittle solid at room temperature and is nonmallable