Chem 1 Chapter 7 part 2 and chapter 8 part 1

Which of the following pairs of ions represent isoelectronic species? A) Na⁺ and N²⁻ B) Al³⁺ and O²⁻ C) K⁺ and Na⁺ D) Cl⁻ and F⁻ E) Al³⁺ and P³⁻

B) Al³⁺ and O²⁻

Which of the following electron configurations is incorrect? A) Ca [Ar]4s² B) Mn [Ar]4s²4d⁵ C) Cu [Ar]4s¹3d¹⁰ D) Ga [Ar]4s²3d¹⁰4p¹ E) Br [Ar]4s²3d¹⁰4p⁵

B) Mn [Ar]4s²4d⁵

Given n = 2, identify which of the quantum numbers is NOT possible. A) l = 1 B) l = 2 C) m(l) = -1 D) m(s) = +½ E) m(s) = -½

B) l = 2

Which of the following sets of quantum numbers is not allowed? A) n = 1, ℓ = 0, mℓ = 0 B) n = 4, ℓ = 0, mℓ = -1 C) n = 3, ℓ = 1, mℓ = 0 D) n = 2, ℓ = 0, mℓ = 0 E) n = 3, ℓ = 2, mℓ = -2

B) n = 4, ℓ = 0, mℓ = -1

Given a particular value of the principal quantum number (n), which quantum number primarily determines the shape of an orbital? A) n B) ℓ C) mℓ D) ms E) ℓm

B) ℓ The shape of an orbital is determined by the number of angular nodes in that orbital, which is given by the quantum number ℓ.

How many core electrons does an atom of beryllium (Be) contain? A) 0 B) 1 C) 2 D) 3 E) 4

C) 2 The electrons in the 1st shell are in the core and the electrons in the outer shell are valence electrons.

Which of the orbital electron configurations is not possible? A) 2s¹ B) 3d¹⁰ C) 4p⁷ D) 4f⁷ E) 2p⁶

C) 4p⁷

Which of the following sets of quantum numbers can describe a 3p electron? A) n = 1, ℓ = 3, mℓ = 1 B) n = 3, ℓ = 2, mℓ = 1 C) n = 3, ℓ = 1, mℓ = 1 D) n = 3 , ℓ = 0, mℓ = 1 E) n = 2, ℓ = 3, mℓ = 1

C) n = 3, ℓ = 1, mℓ = 1

Which of the following orbitals cannot exist? A) 2p B) 3d C) 4d D) 3f E) 162p

D) 3f

Of the following, which sublevel is filled last? A) 3d B) 4s C) 4p D) 4d E) 5s

D) 4d

In a multi-electron atom, which orbital will have the highest energy? A) 4s B) 4p C) 4d D) 4f E) All are equal

D) 4f For atoms with multiple electrons, electrons that have the same value of n (as is the case here, with n = 4) will have higher energies with higher values of ℓ

How many valence electrons are in a neutral atom of nitrogen? A) 0 B) 2 C) 3 D) 5 E) 7

D) 5

How many valence electrons are in a neutral atom of chlorine? A) 0 B) 3 C) 5 D) 7 E) 17

D) 7

Rank the following atoms in order of increasing size (i.e., smallest to largest): Li, Al, Be, Ba, O. A) Li < Al < Be < Ba < O B) Ba < Al < Li < Be < O C) Li < Be < O < Al < Ba D) O < Be < Li < Al < Ba E) O < Li < Be < Ba < Al

D) O < Be < Li < Al < Ba

Rank the following atoms in order of increasing first ionization energies (i.e., lowest to highest): Rb, F, Mg, B, N. A) F < N < B < Mg < Rb B) Rb < Mg < F < N < B C) Mg < Rb < F < N < B D) Rb < Mg < B < N < F E) Rb > B > N > F > Mg

D) Rb < Mg < B < N < F

Atomic radii decrease from left to right in a period (Na → Ar) on the periodic table. Choose the best explanation for this observed trend. A) The ionization potential decreases in that direction. B) The electron affinity increases in that direction. C) The atomic mass increases in that direction. D) The nuclear charge increases in that direction. E) The number of electrons increases in that direction.

D) The nuclear charge increases in that direction.

A single electron occupies a subshell and has the quantum numbers n = 2, ℓ = 1, mℓ = -1, ms = +½. Which of the following is an acceptable set of quantum numbers for the next electron added to this subshell? A) n = 2, ℓ = 1, mℓ = -1, ms = +½ B) n = 2, ℓ = 1, mℓ = -1, ms = -½ C) n = 3, ℓ = 0, mℓ = 0, ms = +½ D) n = 2, ℓ = 1, mℓ = 0, ms = +½ E) n = 2, ℓ = 1, mℓ = 1, ms = -½

D) n = 2, ℓ = 1, mℓ = 0, ms = +½

For an atom of carbon, which ionization will exhibit a very large increase in the energy relative to the preceding ionization? A) 1st B) 2nd C) 3rd D) 4th E) 5th

E) 5th There are four valence electrons in an atom of carbon. The 5th ionization will require a very large increase in the energy relative to the preceding ionization.

Which of the following elements has the smallest first ionization energy? A) S B) O C) Si D) Sr E) Cs

E) Cs

Which of the following metals would be expected to have the smallest atomic radius? A) Cesium (Cs) B) Barium (Ba) C) Lanthanum (La) D) Europium (Eu) E) Tantalum (Ta)

E) Tantalum (Ta)

A single electron occupies a subshell and has the quantum numbers n = 3, ℓ = 0, mℓ = 0, ms = +½. Which of the following is an acceptable set of quantum numbers for the next electron added to this subshell? A) n = 3, ℓ = 1, mℓ = 0, ms = +½ B) n = 3, ℓ = 2, mℓ = 0, ms = +½ C) n = 3, ℓ = 1, mℓ = -1, ms = -½ D) n = 3, ℓ = 0, mℓ = 0, ms = +½ E) n = 3, ℓ = 0, mℓ = 0, ms = -½

E) n = 3, ℓ = 0, mℓ = 0, ms = -½

What is the maximum number of electrons that can have the following set of quantum numbers? n = 4, ℓ = 3, mℓ = 3, ms = -½

1 The Pauli exclusion principle states that no two electrons in a given atom can share the same set of four quantum numbers (n, ℓ, mℓ, ms)

If n = 2, what is the maximum allowed value for ℓ?

1 (p)

In one atom, what is the maximum number of electrons that could have the quantum number of n = 2?

8

Which of the following atoms would have the longest de Broglie wavelength, if all have the same velocity? A) Li B) Na C) Fe D) Pb E) Not possible to tell with given information

A) Li

Rank the following atoms in order of decreasing size (i.e., largest to smallest): Rb, F, Mg, B, N. A) Rb > Mg > B > N > F B) N > F > B > Mg > Rb C) Rb > Mg > F > N > B D) Mg > Rb > B > N > F E) Rb > Mg > N > B > F

A) Rb > Mg > B > N > F

True or false: two electrons can simultaneously occupy the same (n,ℓ,mℓ) orbital. A) True B) False

A) True The Pauli exclusion principle states that no two electrons in a given atom can share the same set of four quantum numbers (nn, ℓℓ, mℓmℓ, msms)

A ground state atom of Mg could not have any electrons with which of the following configurations? A) n = 3, ℓ = 1, mℓ = 0, ms = +½ B) n = 2, ℓ = 1, mℓ = 0, ms = +½ C) n = 3, ℓ = 0, mℓ = 0, ms = +½ D) n = 2, ℓ = 0, mℓ = 0, ms = +½ E) n = 1, ℓ = 0, mℓ = 0, ms = +½

A) n = 3, ℓ = 1, mℓ = 0, ms = +½

If ℓ = 0, which of the following may be true? A) n = 6 B) mℓ = -1 C) mℓ = 1 D) ms = 1 E) ms = 0

A) n = 6

de Broglie equation

λ = h/mv