Honors Chemistry Unit 4 Test
velocity
All electromagnetic radiation travels at the same ________.
alakli metals
All of the __________ have a valence shell electron configuration ns1.
violet, indigo, blue, green, yellow, orange, red
Arrange the colors of light in the visible spectrum in order of decreasing frequency.
Se, Ge, In, Cs
Arrange the elements in decreasing order of first ionization energy: selenium, cesium, germanium, indium
in an atom dropping from one energy level to a lower one.
Atomic emission spectra are due to electrons
Ca
Based on their positions in the periodic table, predict which atom of the following pair will have the smaller first ionization energy:
Cu
Based on their positions in the periodic table, predict which atom of the following pair will have the smaller first ionization energy:
I
Based on their positions in the periodic table, predict which atom of the following pair will have the smaller first ionization energy:
K
Based on their positions in the periodic table, predict which atom of the following pair will have the smaller first ionization energy:
Pb
Based on their positions in the periodic table, predict which atom of the following pair will have the smaller first ionization energy:
waves
Electromagnetic radiation normally travels in the form of ________.
increases, decreases
Electronegativity __________ from left to right within a period and __________ from top to bottom within a group.
8A
Elements in group __________ have a np6 electron configuration in the outer shell.
atomic number
Elements in the modern version of the periodic table are arranged in order of increasing __________.
2,4,2 electrons
For each element, count the number of core electrons, valence electrons, and unpaired electrons in the ground state. carbon
2,8,0 electrons
For each element, count the number of core electrons, valence electrons, and unpaired electrons in the ground state. neon
10,5,3 electrons
For each element, count the number of core electrons, valence electrons, and unpaired electrons in the ground state. phosphorus
element x, element y, element z
For the series of elements X, Y, and Z all in the same period (row), arrange the elements in order of decreasing first ionization energy.
c= λ × ν (c - the speed of light)
How are the wavelength (λ) and frequency (ν) of light related?
1
How many UNPAIRED electrons are in the ground state electron configuration for boron?
2
How many UNPAIRED electrons are in the ground state electron configuration for carbon?
3
How many UNPAIRED electrons are in the ground state electron configuration for phosphorous?
9
How many orbitals are there in the third shell (n=3)?
Be
Identify the specific element that corresponds to each of the following electron configurations. 1s2 2s2
O
Identify the specific element that corresponds to each of the following electron configurations. 1s2 2s2 2p4
Cr
Identify the specific element that corresponds to each of the following electron configurations. [Ar]4s1 3d5
Te
Identify the specific element that corresponds to each of the following electron configurations. [Kr]5s2 4d10 5p4
4d
In a ground-state rhodium atoms, the __________ subshell is partially filled.
1+,2+
In their compounds, the charges on the alkali metals and the alkaline earth metals are __________ and __________, respectively.
O, S, Se
In which set of elements would all members be expected to have very similar chemical properties?
radio waves
Infrared radiation has a shorter wavelength than ________.
the energy required to remove an electron from the ground state of a neutral gaseous atom or ion.
Ionization energy is:
B
Of the atoms below, __________ is the least electronegative.
Cl
Of the atoms below, __________ is the most electronegative.
Li
Of the atoms below, __________ is the most electronegative.
Ar > Cl > S > Si > Al
Of the choices below, which gives the order for first ionization energies?
H
Of the following atoms, which has the largest first ionization energy?
N
Of the following atoms, which has the largest first ionization energy?
Na > Mg > Si > P > Ar
Of the following, which gives the correct order for atomic radius for Mg, Na, P, Si and Ar?
1s^22s^22p^63s^23p^64s^23d^104p^65s^04d^10
Pd has an anomalous electron configuration. Write the observed electron configuration of Pd.
Cs, Ba, Bi, As, Br, Ne
Place the following elements in order of decreasing atomic size: bismuth, bromine, neon, cesium, barium, and arsenic.
Cs, Sr, Te, Se, Br, Ar
Place the following elements in order of decreasing atomic size: tellurium, bromine, argon, cesium, strontium, and selenium.
B, C, O, F
Rank the following elements in order of decreasing atomic radius. B, F, O, C
Sr, Ca, Mg, Be
Rank the following elements in order of decreasing atomic radius. Sr, Mg, Be, Ca
Ga
State where in the periodic table these elements appear: an element whose valence electrons are 4s24p1
group 15
State where in the periodic table these elements appear: elements that have three unpaired p electrons
halogens
State where in the periodic table these elements appear: elements with the valence-shell electron configuration ns2np5
groups 3-12
State where in the periodic table these elements appear: the d-block elements
2
The 3p subshell in the ground state of atomic silicon contains __________ electrons.
6
The 3p subshell in the ground state of atomic xenon contains __________ electrons.
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p3
The complete electron configuration of arsenic, element 33, is __________.
[Ar]3d10 4s2 4p3
The condensed electron configuration of arsenic, element 33, is __________.
[Ne]3s1
The condensed electron configuration of sodium, element 11, is __________.
carbon
The element that corresponds to the electron configuration 1s^22s^22p^2 is __________.
third
The elements in the __________ period of the periodic table have a core-electron configuration that is the same as the electron configuration of neon.
increase, increase
The first ionization energies of the elements __________ as you go from left to right across a period of the periodic table, and __________ as you go from the bottom to the top of a group in the table.
Se; [Ar]4s^23d^104p^4
The following electron configurations represent excited states. Identify the element, and write its ground-state condensed electron configuration. [Ar]3d10 4s1 4p4 5s1
Rh; [Kr]5s^14d^8
The following electron configurations represent excited states. Identify the element, and write its ground-state condensed electron configuration. [Kr]4d65s25p1
N; [He]2s^22p^3
The following electron configurations represent excited states. Identify the element, and write its ground-state condensed electron configuration. ls2 2s2 3p2 4p1
[He]2s2 2p5
The ground state configuration of fluorine is __________.
[Ar] 4s2 3d10
The ground state electron configuration for Zn is __________.
1s2 2s2 2p6 3s2 3p64s2 3d10 4p1
The ground state electron configuration of Ga is __________.
4
The largest principal quantum number in the ground state electron configuration of cobalt is __________.
frequency
The number of electromagnetic waves that travel past a certain point in a given time is the ________ of the radiation.
8
The second shell in the ground state of atomic argon contains __________ electrons.
+3 and +6
The shielding of electrons gives rise to an effective nuclear charge, Zeff, which explains why boron is larger than oxygen. Estimate the approximate Zeff felt by a valence electron of boron and oxygen, respectively?
photon
The smallest particle of light is called a ________.
λ
The symbol for wavelength of electromagnetic radiation is ________.
transition metal
The valence shell of the element X contains 2 electrons in a 5s subshell. Below that shell, element X has a partially filled 4d subshell. What type of element is X?
400 to 700 nm
The visible light spectrum covers the wavelength range ________.
3
There are __________ unpaired electrons in a ground state phosphorus atom.
1s^22s^22p^63s^23p^64s^2
Use the rules for determining electron configurations to write the electron configuration for Ca.
2s, 2p, 3s, 3p, 3d, 4s
Using only a periodic table, identify which set of electron sublevels is NOT organized from lowest energy to highest energy. -2s, 2p, 3s, 3p, 3d, 4s -1s, 2s, 2p, 3s, 3p, 4s -2s, 2p, 3s, 3p, 4s, 3d -5s, 4d, 5p, 6s, 4f, 5d
the number of valence electrons
What do the group numbers from 1A to 8A for the elements indicate about electron configurations of those elements? -the total number of electrons -the number of energy sublevels -the number of valence electrons -the total number of protons -none of these
[Ar]3d^84s^2
What is the ground-state electron configuration of a neutral atom of nickel?
[Ne]
What is the ground-state electron configuration of the fluoride ion F−?
2
What is the maximum number of electrons that can occupy each of the following subshells? 2s
6
What is the maximum number of electrons that can occupy each of the following subshells? 3p
14
What is the maximum number of electrons that can occupy each of the following subshells? 4f
10
What is the maximum number of electrons that can occupy each of the following subshells? 5d
10
What is the maximum number of electrons that can occupy the 3d sublevel? *
visible light
What portion of the electromagnetic spectrum can our eyes detect?
radio waves
What type of radiation has the longest wavelength?
2s
When electrons are removed from a lithium atom they are removed first from which orbital?
moves from a lower to a higher energy level.
When ultraviolet energy is absorbed by an atom, an electron
violet
Which color of light has the greatest energy?
red
Which color of light has the longest wavelength?
C
Which diagram has the lowest frequency?
A
Which diagram has the shortest wavelength?
the first one
Which electron configuration denotes an atom in its ground state?
the last one
Which electron configuration represents a violation of Hund's rule for an atom in its ground state?
the first one
Which electron configuration represents a violation of the Pauli exclusion principle?
the last one
Which electron configuration represents a violation of the Pauli exclusion principle?
Na
Which element fits the following description: an element that has 1 electron in the n = 3 energy level?
B
Which element fits the following description: an element that has 3 electrons in the n = 2 energy level?
Mg
Which element has atoms with the smallest ionization energy? -Al -Ar -Cl -Mg -P
Ar
Which element has atoms with the smallest radius? -Al -Ar -Cl -Mg -P
Gd
Which element has the following configuration: [Xe]6s24f75d1?
Rb
Which element has the largest atomic radius? -K -He -Rb -Xe -all have the same radius
Li
Which element has the lowest electronegativity? -Li -C -N -O -F
Na
Which element has the lowest ionization energy? -Cl -P -Si -Mg -Na
Al
Which element has this electron configuration?
Xe
Which element would be expected to have chemical and physical properties closest to those of krypton?
Ru
Which element would have 4d^6 as the last entry of its electron configuration?
Al(g)→Al⁺(g)+e⁻
Which equation correctly represents the first ionization of aluminum?
P(g)→P⁺(g)+e⁻
Which equation correctly represents the first ionization of phosphorus?
3A
Which group in the periodic table contains elements with the valence electron configuration of ns2np1?
Energy is a minimum when the number of same-spin electrons is maximized.
Which is a statement of Hund's rule?
Uranium is an example of an actinide element.
Which is true about the actinides?
Se
Which neutral element has this excited state electron configuration?
He
Which noble gas has the highest first ionization energy?
helium
Which noble gas has the highest first ionization energy?
F < Br < Ge < K < Rb
Which of the following correctly lists the five atoms in order of increasing size (smallest to largest)?
F < Cl < Br
Which of the sets of elements are NOT in order of INCREASING force of attraction on the outermost electron in atoms of that element? -Ba < Sr < Ca -Al < P < Cl -F < Cl < Br -Mo < Pd < Sn -all sets are in the correct order
1s2 2s2 2p1 3s1
Which one of the following configurations depicts an excited carbon atom?
1s2 2s2 2p2 3s2
Which one of the following configurations depicts an excited oxygen atom?
Al
Which one of the following has the smallest radius?
the third one
Which one of the following is the correct electron configuration for a ground-state nitrogen atom?
B
Which orbital diagram represents a boron atom in the ground state?
S < C
Which pair correctly ranks the electronegativities of the atoms?
O > Br > Mg > Ba
Which set has the correct order of decreasing first ionization energy?
Al³⁺, Mg²⁺, Na⁺
Which set has the same number and same configuration of its electrons?
Set A
Which set of particles has the GREATEST force of attraction on the electron?
Set C
Which set of particles has the LEAST force of attraction on the electron?
No two elements have the same ground-state electron configuration.
Which two elements have the same ground-state electron configuration?
[Xe]6s^2
Write the condensed electron configurations for the following atoms, using the appropriate noble-gas core abbreviations. Ba
[Kr]5s^24d^10
Write the condensed electron configurations for the following atoms, using the appropriate noble-gas core abbreviations. Cd
[Xe]6s^1
Write the condensed electron configurations for the following atoms, using the appropriate noble-gas core abbreviations. Cs
[Ar]4s^23d^8
Write the condensed electron configurations for the following atoms, using the appropriate noble-gas core abbreviations. Ni
[Xe]6s^24f^145d^106p^2
Write the condensed electron configurations for the following atoms, using the appropriate noble-gas core abbreviations. Pb
[Ar]4s^23d^104p^4
Write the condensed electron configurations for the following atoms, using the appropriate noble-gas core abbreviations. Se
Alkali metals
__________ have the lowest first ionization energies of the groups listed.
attraction, stronger
as an electron gets closer to the nucleus, the _________ to the nucleus gets ________
decreases
as photon energy increases, wavelength _______________
decreases
as you move across the periodic table, the attractive force of the outermost electron in an atom ________________
increases
as you move down the periodic table, the attractive force of the outermost electron in an atom ________________
see picture
convert the frequency of the following metals to Hz(1THz = 1 x 10¹² Hz). Then calculate the wavelength of the light emitted, converting to nm(1nm=1 x 10⁻⁹m).
see picture
convert the wavelenth to meters (1nm=1 x 10⁻⁹m); then calculate the frequency of the light emitted and convert to THZ(1THz = 1 x 10¹² Hz) barium -- 550 nm
as you go down a group, ionization energy decreases because as the atomic radius increases, the force of attraction between electrons and the nucleus decreases, resulting in less energy being required to remove electrons
describe why the ionization energy of atoms decreases as you go down a group
as you go across a period, ionization energy increases because as the atomic radius decreases, the force of attraction between electrosn and the nucleus increases, resulting in more energy being required to remove electrons
describe why the ionization energy of atoms increases as you go across a period
3p ↑ 3s ↑↓ 2p ↑↓ ↑↓ ↑↓ 2s ↑↓ 1s ↑↓
draw a ground state orbital diagram for Al
3p ↑↓ ↑↓ ↑↓ 3s ↑↓ 2p ↑↓ ↑↓ ↑↓ 2s ↑↓ 1s ↑↓
draw a ground state orbital diagram for Ar
2p ↑ 2s ↑↓ 1s ↑↓
draw a ground state orbital diagram for B
2s ↑↓ 1s ↑↓
draw a ground state orbital diagram for Be
2p ↑ ↑ 2s ↑↓ 1s ↑↓
draw a ground state orbital diagram for C
3p ↑↓ ↑↓ ↑ 3s ↑↓ 2p ↑↓ ↑↓ ↑↓ 2s ↑↓ 1s ↑↓
draw a ground state orbital diagram for Cl
2p ↑↓ ↑↓ ↑ 2s ↑↓ 1s ↑↓
draw a ground state orbital diagram for F
1s ↑
draw a ground state orbital diagram for H
1s ↑↓
draw a ground state orbital diagram for He
2s ↑ 1s ↑↓
draw a ground state orbital diagram for Li
3s ↑↓ 2p ↑↓ ↑↓ ↑↓ 2s ↑↓ 1s ↑↓
draw a ground state orbital diagram for Mg
2p ↑ ↑ ↑ 2s ↑↓ 1s ↑↓
draw a ground state orbital diagram for N
3s ↑ 2p ↑↓ ↑↓ ↑↓ 2s ↑↓ 1s ↑↓
draw a ground state orbital diagram for Na
2p ↑↓ ↑↓ ↑↓ 2s ↑↓ 1s ↑↓
draw a ground state orbital diagram for Ne
2p ↑↓ ↑ ↑ 2s ↑↓ 1s ↑↓
draw a ground state orbital diagram for O
3p ↑ ↑ ↑ 3s ↑↓ 2p ↑↓ ↑↓ ↑↓ 2s ↑↓ 1s ↑↓
draw a ground state orbital diagram for P
3p ↑↓ ↑ ↑ 3s ↑↓ 2p ↑↓ ↑↓ ↑↓ 2s ↑↓ 1s ↑↓
draw a ground state orbital diagram for S
3p ↑ ↑ 3s ↑↓ 2p ↑↓ ↑↓ ↑↓ 2s ↑↓ 1s ↑↓
draw a ground state orbital diagram for Si
release
electrons _______ energy as they move from high energy levels to low energy levels
absorb
electrons _______ energy as they move from low energy levels to high energy levels
these lines come from photons of a specific energy, emitted by electrons making transitions between specific energy levels of the atom.
explain how the lines in an emission spectrum relate to the energy levels of electrons in an atom
the atomic radii decreases as you go across a period (L → R) because the highest energy level remains constant, but the # of protons in the nucleus increases, increasing the charge of the nucleus and attractive force on the electrons, pulling the highest energy level closer to the nucleus
explain why the atomic radii of atoms decreases across a period using knowledge of atomic structure and coulombic attraction
the atomic radii increases as you go down a group because as the number of electrons increases, new energy levels are need to be added further from the nucleus, increasing the radius
explain why the atomic radii of atoms increases down a group using knowledge of atomic structure and coulombic attraction
gain
for an electron to move from an energy level close to the nucleus to an energy level far from the nucleus, it would need to ______ energy
lose
for an electron to move from an energy level far from the nucleus to an energy level close to the nucleus, it would need to _______ energy
main group number
for neutral atoms, the number of valence electrons is equal to the atom's
c=λν
formula to convert between wavelength and frequency
increases as you go L → R decrease as you go top to bottom
predict the trend in electronegativity of atoms across a period and down a group using knowledge of atomic structure and coulombic attraction
C, B, A
rank these in order of increasing force of attraction
F, E, D, A
rank these in order of increasing force of attraction
lower
the longer the wavelength, the ___________ the frequency
10
the max number of electrons in the d orbital is
14
the max number of electrons in the f orbital is
6
the max number of electrons in the p orbital is
2
the max number of electrons in the s orbital is
higher
the shorter the wavelength, the ___________ the frequency
gamma ray x-ray ultraviolet visible light infrared microwave radio wave
what's the electromagnetic spectrum
