Unit 2 Review Questions

Electrons are elevated from the ground state to the excited state by:
1. the release of energy
2. the absorption of energy
3. the loss of mass
4. the destruction of energy
When a salt such as sodium chloride is exposed to a flame, the visible light given off is the result of:
1. ground state electrons moving to higher energy levels
2. excited electrons returning to the ground state
3. nuclear decay
4. gamma radiation
The Principal quantum number (n) of an electron indicates the:
1. spin of the electron
2. energy level (shell) of the electron
3. mass of the electron
4. charge of the electron
How many electrons can fit in the third energy level?
1. 3
2. 8
3. 18
4. 32
5. n²
The electron configuration notation for the element of atomic number 5 is:
1. 1s²2s²2p¹
2. 1s²2s¹2p²
3. 1s²2p³
4. 1s⁵
The number of electrons that may occupy any orbital is:
1. 2
2. 6
3. 10
4. 14
The maximum number of electrons that may occupy a 3d sublevel is:
1. 10
2. 5
3. 6
4. 2
Which of the following is the correct configuration notation for the element titanium (Ti, atomic number 22)?
1. 1s²2s²2p⁶3s²3p⁶4s²3d²
2. 1s²2s²2p⁶3s²3p⁶4s²4d²
3. 1s²2s²2p⁶3s²3p⁶3d²4s²
4. 1s²2s²2p⁶3s²3p⁶4s²1d²
Which of the following is the correct noble-gas notation for the element strontium (Sr, atomic #38)?
1. [Kr]5s²
2. [Kr]6s²
3. [Xe]5s²
4. [Kr]5s¹
What element has the noble-gas notation [Ne]3s²3p⁵?
1. Sulfur
2. Oxygen
3. Chlorine
4. Neon
What element has the configuration notation 1s²2s²2p⁴?
1. Nitrogen
2. Oxygen
3. Fluorine
4. Neon
What element has the electron configuration notation 1s²2s²2p⁶3s¹?
What element has the noble gas configuration [Ne]3s²3p¹?
Which of the following is the correct orbital notation for the element oxygen (O, atomic #8)?
Which of the following is the correct orbital notation for the 3d sublevel of the element nickel, (Ni, atomic #28).
The orbital notation depicted here is for the element:
The "up" and "down" arrows in electron orbital notation, such as is shown here, depict:
1. electrons and protons attracting each other
2. electrons with opposite spins
3. oppositely charged electrons
4. protons and neutrons in orbitals
The noble-gas notation for the element indium, (In, atomic #49) is:
1. [Kr]5s²4d¹⁰5p¹
2. [Kr]5s²5d¹⁰5p¹
3. [Kr]5s²4f¹⁴5d¹⁰5p¹
4. [Kr]5p¹
Which of the following is the correct orbital notation for the element carbon, (C, atomic #6)?
What element has the noble-gas notation [Xe]6s²?
An atom or a group of atoms that has a net positive or negative charge is a(n):
1. isotope
2. ion
3. radical
4. orbital
A horizontal row of elements on the Periodic Table is known as a(n):
1. group or family
2. atomic number
3. period or series
4. size
The elements on the modern periodic table are organized by increasing:
1. atomic mass
2. atomic number
3. ionization energy
4. size
The elements of the Noble Gas family, except for Helium, have an outer shell of:
1. 2 electrons
2. 6 electrons
3. 8 electrons
4. 18 electrons
As the atomic number of the elements in Group II increase, the atomic radius of the successive elements:
1. increases only
2. decreases only
3. increases then decreases
4. remains the same
Of the following groups, which would have the highest first ionization energy?
1. Group 1
2. Group 2
3. Group 17
4. Group 18
In the third period, as the atomic number increases from Group 1 to Group 18, the atomic radius:
1. increases only
2. decreases only
3. increases then decreases
4. remains the same
According to the modern periodic law, the chemical properties of the elements are periodic functions of their:
1. atomic mass
2. atomic weight
3. atomic number
4. isotopic weight
Metalloids are elements that show:
1. properties of the Noble Gases
2. only properties of metals
3. both metallic and nonmetallic properties
4. only properties of nonmetals
For each successive electron removed from an atom, the ionization energy:
1. increases
2. decreases
3. remains the same
Low ionization energies are most characteristic of:
1. Noble gases
2. Halogens
3. Metalloids
4. Metals
An element with the electron configuration 1s²2s²2p⁵ belongs to the:
1. alkali metal group
2. transition metal group
3. alkaline earth metal group
4. halogen group
5. nobel gas group
The most reactive metals on the periodic table belong to the:
1. Alkali metals group
2. Rare earth metals
3. Transition metals
4. Alkaline earth metals group
5. Noble gases
The most active of the following four elements in the Halogen family is:
1. fluorine
2. chlorine
3. bromine
4. iodine
The energy required to remove an electron from an atom is known as:
1. electron affinity
2. electronegativity
3. radioactivity
4. ionization energy
The measure of the attraction that an atom has for electrons involved in chemical bonds is known as:
1. electron affinity
2. electronegativity
3. radioactivity
4. ionization energy
The most active metals are located in the:
1. lower right hand corner of the periodic table
2. lower left hand corner of the periodic table
3. upper right hand corner of the periodic table
4. upper left hand corner of the periodic table
Transition elements are classified as:
1. metals
2. nonmetals
3. metalliods
4. semiconductors
Which of the following changes would result in the greatest shrinkage in atomic radius?
1. Gaining one electron to form a 1- anion
2. Gaining two electrons to form a 2- anion
3. Losing one electron to form a 1+ cation
4. Losing two electrons to form a 2+ cation
The least electronegative elements are the:
1. Noble gases
2. Alkali metals
3. Halogens
4. Metalloids
The elements with the largest atomic radii are found in the:
1. upper right-hand corner of the periodic table
2. upper left-hand corner of the periodic table
3. lower right-hand corner of the periodic table
4. lower left-hand corner of the periodic table
The elements with the smallest atomic radii are found in the:
1. upper right-hand corner of the periodic table
2. upper left-hand corner of the periodic table
3. lower right-hand corner of the periodic table
4. lower left-hand corner of the periodic table
Anions have a ______________ charge and are ______________ than the atoms from which they formed.
1. positive/larger
2. positive/smaller
3. negative/larger
4. negative/smaller
Cations have a ______________ charge and are ______________ than the atoms from which they formed.
1. positive/larger
2. positive/smaller
3. negative/larger
4. negative/smaller
Given the representation of a chlorine atom, which circle might represent an atom of argon?
1. None of these
2. Circle B
3. Circle C
4. Circle D
Given the representation of a chlorine atom, which circle might represent an atom of sulfur?
1. None of these
2. Circle B
3. Circle C
4. Circle D
Given the representation of a chlorine atom, which circle might represent an atom of fluorine?
1. None of these
2. Circle B
3. Circle C
4. Circle D
Given the representation of a chlorine atom, which circle might represent an atom of bromine?
1. None of these
2. Circle B
3. Circle C
4. Circle D
Given the representation of a chlorine atom, which circle might a chloride ion, Cl^-?
1. None of these
2. Circle B
3. Circle C
4. Circle D
Which of the following elements is a noble gas?
1. Oxygen, atomic #8
2. Chlorine, atomic #17
3. Radium, atomic #88
4. Krypton, atomic #36
Which of the following elements is a halogen?
1. Iron(#26)
2. Germanium(#32)
3. Sulfur(#16)
4. Potassium(#19)
5. Iodine(#53)
Which of the following elements is a transition metal?
1. Iron(#26)
2. Germanium(#32)
3. Sulfur(#16)
4. Potassium(#19)
5. Iodine(#53)
Which of the following elements is a alkali metal?
1. Iron(#26)
2. Germanium(#32)
3. Sulfur(#16)
4. Potassium(#19)
5. Iodine(#53)
Which of the following elements is a metalloid?
1. Iron(#26)
2. Germanium(#32)
3. Sulfur(#16)
4. Potassium(#19)
5. Iodine(#53)
Which of the following elements is a nonmetal?
1. Iron(#26)
2. Germanium(#32)
3. Sulfur(#16)
4. Potassium(#19)
5. Iodine(#53)
Which of these elements is a halogen?
1. Element A
2. Element B
3. Element C
4. Element D
Which of these elements would have the lowest first ionization energy?
1. Element A
2. Element B
3. Element C
4. Element D
Element B is an:
1. alkali metal
2. alkaline earth metal
3. transition metal
4. halogen

Electron Review Questions

Multiple-choice exercise