chemistry exam 2

What is the value of ℓ for the orbital shown below (The orbital shown in this figure has one angular node)

1

n a ground state atom of Ar how many electrons total will have the quantum number ℓ = 0?

6 --- 1s, 2s, 3s, each having 2 electrons

Predict the chemical formula for the ionic compound formed by the elements Ba and S

BaS -- Ba has a +2 charge and S has a -2 charge.--

What scientist proposed that the electron in a hydrogen atom can only have certain energies (i.e., the electron is quantized)?

Bohr

Predict the chemical formula for the ionic compound formed by the elements Ca and Br

CaBr2 -- Ca has a 2+ charge and Br has a 1- charge, you need two Br to get a 2- charge in order to cancel out the charges and get them to equal zero--

What is the correct IUPAC name for CrN?

Chromium (III) nitride

What is the correct IUPAC name for Cu₂S?

Copper(I) Sulfide

Which of the following sets of quantum numbers could describe an electron in the orbital shown below? (a big circle) a. n=3, l=2, ml=-2 b. n=2, l=1, ml=-1 c. n=3, l=1, ml=0 d. n=3, l=0, ml=0 e. n=4, l=1, ml=1

D) n = 3, ℓ = 0, mℓ = 0

Which of the following is true concerning successive ionizations of an atom and its ions? a. each successive ionization requires less energy to achieve b. all ionization require the same amount of energy c. the amount of energy to achieve a successive ionization doubles with each electron removed d. each successive ionization requires increasing amounts of energy e. the first two ionizations are endothermic but each ionization afterwards is exothermic

D. Each successive ionization requires increasing amounts of energy.

A Lewis structure with placeholder central atom is shown below. If the charge of the molecule is -1, choose the possible identity or identities of the central atom. A. F B. N, P or As C. C, Si, or Ge D. B or Al E. Cl, Br, or I

E. Cl, Br, or I

Which one of the following is the most electronegative atom? a.C b.N c.O d.F

F

Rank the following atoms in order of decreasing first ionization energies (i.e., highest to lowest): Li, Be, Ba, F.

F>Be>Li>Ba

What is the correct IUPAC name for Ir(OH)₃?

Iridium (III) hydroxide

Which of the following does NOT describe the element bromine (Br)? a. A metalloid b. A nonmetal c.A main group element d. A halogen

a. A metalloid

Which periodic trend quantifies the amount of energy required to remove an electron from a neutral, gaseous atom? a. atomic radius b. ionization energy c. ionic radius d. electron affinity e. electronegativity

b. Ionization Energy

Which of the following is not a property affected by the effective nuclear charge, Zeff? a. ionization energy b. color c. electron affinity d. atomic radius e. ionic radius

b. color

The first five ionization energies of an element are as follows (in kJ/mol): 577.9, 1820, 2750, 11600, 14800. Which of the following elements is most likely to have these ionization energy values? a. Na b. Mg c. Al d. Si e. P

c. Al

Based on their positions in the periodic table, which of the following bonds is the most polar? A. O-F B. C-F C. B-F D. F-F

c. B-F

Which of the following states that no two electrons can have the same set of four quantum numbers? a. Hunds rule b. de brogues wave equation c. Pauli exclusion principle d. Bohr equation e. Schrödinger equation

c. Pauli exclusion principle

Which element has the ground state electron configuration [Kr]5s²4d¹⁰5p³? a.Te b.Pb c.Sb d.Bi e.Sn

c. Sb

Which of the following sets of quantum numbers is not allowed? a. n=2, l=0, ml=0 b. n=3, l=2, ml=0 c. n=2, l=2, ml=2 d. n=3, l=1, ml=-1 e. n=4, l=2, ml=1

c. n=2, l=2, ml=2 - the value of l cannot be the same as n

Which of the following sets of quantum numbers can describe a 3p electron? a. n=3, 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

What is the correct IUPAC name for Cs₃P?

cesium phosphide

Which of the following orbitals cannot exist? a.2p b.3d c. 4d d. 3f e. 162p

d. 3f

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

Classify the following compounds as ionic or covalent: BaO, Fe₂O₃, ZnO. a. covalent, covalent, covalent b. ionic, ionic, covalent c. ionic, covalent, covalent d. ionic, ionic, ionic

d. ionic, ionic, ionic

Which diatomic molecule has the smallest dipole moment? a. F2 b. O2 c. N2 d.H2 e. All equal

e. All equal Homonuclear molecules do not have charge separation between the identical nuclei and therefore contain no dipole moments.

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) -- The atomic radius increases as you move down the periodic table and to the left.

ionization energy___________ across a period and ____________ down a group

increases, decreases

What is the correct IUPAC name for FeCl₃ · 6H₂O?

iron (III) chloride hexahydrate

What is the correct IUPAC name for SCl₂?

sulfer dichloride

What is the correct IUPAC name for P₄S₃?

tetraphosphorous disulfide

Which group in the periodic table tends to have high electronegativity values? a. the alkali metals b. the noble gases c. the halogens d. the transition metals

the halogens

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

true

In which direction on the periodic table does metallic character increase? a. Down and to the right b. Down and to the left c. As you move toward the middle of the table d. Up and to the right e. Up and to the left

b. down and to the left

What is the electron configuration of K⁺?

1s²2s²2p⁶3s²3p⁶

Which of the following represents the electron configuration of P³⁻?

1s²2s²2p⁶3s²3p⁶

The ground state electron configuration of a Se atom is

1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁴

Which of the following is the electron configuration of a neutral Fe atom?

1s²2s²2p⁶3s²3p⁶4s²3d⁶

How many orbitals are allowed in the subshell when ℓ = 2?

5 -2, -1, 0, 1, 2

A student draws the orbital diagram below for the 3d electrons in a V atom. What, if anything, is incorrect about the drawing? {^v}{^ }{ }{ }{ } 3d a. It violates the aufbau principle b. it violates the pauli exclusion principle c. it violates the heisenburg uncertainty principle d. it violates hunds rule e. there is nothing wrong about the picture

d. It violates hunds rule ---Hund's rule states that electrons are added to the atomic orbitals with the same energy levels (degenerate orbitals) in such a way that each orbital is occupied by a single electron with the same spin (either +½ or -½) before any orbital can be occupied by two electrons.---

Effective nuclear charge, Zeff, is defined as a. the number or protons minus the number of valance electrons b. the difference in electronegative of two bonded atoms or ions c. the number of protons minus the number of electrons d. the true nuclear charge minus the charge that is sheild by electrons e. the number of protons in the nucleus

d. the true nuclear charge minus the charge that is shielded by electrons.