Q&A Hero

Q: Which of the above pictures are more likely to represent ionic compounds?A) pictures (a) and (b)B) pictures (a) and (d)C) pictures (b) and (c)D) pictures (b) and (d)

Q: Which of the above pictures best represents a gaseous covalent compound?A) picture (a)B) picture (b)C) picture (c)D) picture (d)

Q: Which of the above pictures best represents a solid ionic compound?A) picture (a)B) picture (b)C) picture (c)D) picture (d)

Q: Which of the above drawings represents a K+ ion?A) drawing (a)B) drawing (b)C) drawing (c)D) drawing (d)

Q: Which of the above drawings represents a Ca2+ ion? A) drawing (a) B) drawing (b) C) drawing (c) D) drawing (d)

Q: Which of the above drawings represents a Cl- ion? A) drawing (a) B) drawing (b) C) drawing (c) D) drawing (d)

Q: Which of the above drawings represents an Ar atom?A) drawing (a)B) drawing (b)C) drawing (c)D) drawing (d)

Q: Which elements commonly form covalent bonds?A) A and BB) A and CC) B and DD) C and D

Q: Which elements commonly form cations? A) A and B B) A and C C) B and D D) C and D

Q: Use the periodic table below to answer the following questions.Which elements commonly form anions?A) A and BB) A and CC) B and DD) C and D

Q: Which statement is inconsistent with the chemistry of the noble gases?A) Both helium and radon are radioactive.B) Helium and neon are both lighter than air.C) Neon and argon are used in decorative or designer lights.D) Xenon and krypton react with fluorine to form fluorides.

Q: Which of the following statements about helium is inconsistent with its chemistry? A) A helium oxygen mixture is used as a deep-sea diving gas instead of compressed air. B) In its liquid form it is used as a cryogenic coolant for superconductors. C) It is one of the more reactive elements of its group. D) Its melting point is -272.2C and its boiling point is -268.9C.

Q: Which of the hydrogen halide acids is used to etch glass? A) HF B) HCl C) HBr D) HI

Q: Metals tend to react with the halogens to form metal halides. What is the reactivity order for the halogens? A) F2 > Cl2 > Br2 > I2 B) Cl2 > F2 > Br2 > I2 C) Br2 > I2 > Cl2 > F2 D) I2 > Br2 > Cl2 > F2

Q: Which group of elements are found as diatomic molecules? A) alkali metals B) alkaline earth metals C) halogens D) noble gases

Q: Which of the following elements is a solid at room temperature? A) fluorine B) chlorine C) bromine D) iodine

Q: Which of the following elements is a liquid at room temperature? A) fluorine B) chlorine C) bromine D) iodine

Q: Predict the product(s) when the reactants Be(s) + Br2(l) are mixed. A) BeBr(s) B) BeBr2(s) C) Be2Br(s) D) BeBr3(s)

Q: Group 2A metals tend to be somewhat less reactive than alkali metals, and the order of their reactivity is A) Ba > Sr > Ca > Mg > Be. B) Be > Mg > Ca > Sr > Ba. C) Ca > Mg > Be > Ba > Sr. D) Sr > Ca > Mg > Be > Ba.

Q: Which alkaline earth metal reacts the most vigorously with water at room temperature? A) Be B) Ca C) Ba D) Sr

Q: Which is not generally considered to be a chemical reaction of the alkaline earth metal magnesium?A) 2 Mg(g) + O2(g) -> 2 MgO(s) at room temperatureB) 3 Mg(s) + N2(g) -> Mg3N2(s) at elevated temperaturesC) Mg(s) + 2 H2O(l) -> Mg(OH)2(s) + H2(g) at room temperatureD) Mg(s) + F2(g) -> MgF2(s) at room temperature

Q: Which is not generally considered to be a chemical reaction of the alkaline earth metal calcium?A) Ca(s) + Cl2(g) -> CaCl2(s)B) 2 Ca(s) + 2 H2O(l) -> 2 Ca(OH)2(aq) + H2(g)C) 6 Ca(s) + 2 N2(g) -> 2 Ca3N2(s)D) Ca(s) + O2(g) -> CaO2(s)

Q: Which of the following statements is incorrect about the alkaline earth metals? A) Melting points generally decrease as one descends the group. B) Densities are less than those of the corresponding alkali elements of the same period. C) Ionic radii of the M2+ ion increases as one descends the group. D) The first ionization energy is less than that of the second ionization energy.

Q: Which is not a chemical reaction of the alkali metal sodium?A) 4 Na(s) + 2 O2(g) -> 2 Na2O(s) + Na2O2(s)B) 2 Na(s) + 2 NH3(l) -> 2 NaNH2(sol) + H2(g)C) 2 Na(s) + Cl2(g) -> 2 NaCl(s)D) 2 Na(s) + 2 H2O(l) -> 2 NaOH(aq) + H2(g)

Q: Which alkali metal forms preferentially a peroxide and superoxide? A) Li B) Na C) K D) Mg

Q: Which alkali metal forms preferentially an oxide rather than a peroxide or superoxide? A) Li B) Na C) K D) Rb

Q: The chemical formula for potassium peroxide is A) KOH. B) KO2. C) K2O. D) K2O2.

Q: The compound, Cu(ClO3)2, is named A) copper chlorate(II). B) copper(I) chlorate. C) copper(I) chlorate(II). D) copper(II) chlorate.

Q: KH2PO4 is A) hydropotassium phosphate. B) potassium dihydrogen phosphate. C) potassium diphosphate. D) potassium hydrogen(II) phosphate.

Q: What is the chemical formula for iron(II) phosphate? A) Fe2P B) Fe2PO4 C) Fe3P2 D) Fe3(PO4)2

Q: What is the chemical formula for strontium hydroxide? A) SrH2 B) SrOH C) SrOH2 D) Sr(OH)2

Q: The ions ClO4-, ClO3-, ClO2-, and ClO- are named respectively A) hypochlorate, chlorate, chlorite, perchlorite. B) hypochlorite, chlorite, chlorate, perchlorate. C) perchlorate, chlorate, chlorite, hypochlorite. D) perchlorite, chlorite, chlorate, hypochlorate.

Q: The ion NO2- is named A) nitrate ion. B) nitrite ion. C) nitrogen dioxide ion. D) nitrogen(II) oxide ion.

Q: The thiosulfate ion is A) HS-. B) HSO42-. C) SO52-. D) S2O32-.

Q: The chemical formula for the sulfite ion is A) S-. B) S2-. C) SO32-. D) SO42-.

Q: The chemical formula for calcium nitride is A) Ca(NO3)2. B) Ca(NO2)2. C) Ca3N2. D) CaN2.

Q: What is the chemical formula for strontium hydride? A) SrH2 B) SrOH C) SrOH2 D) Sr(OH)2

Q: The correct chemical formula for manganese(IV) acetate is A) Mn(C B) Mn( C) Mn( D) Mn(

Q: The correct name for Mn(C is A) manganese(IV) acetate B) manganese(II) acetate C) manganese(1V) carbonate D) manganese(II) carbonate

Q: Li2S is named A) lithium disulfide. B) lithium sulfide. C) lithium(II) sulfide. D) lithium sulfur.

Q: What is the charge on the Cr in the ionic compound Cr2O3? A) 2- B) 1+ C) 2+ D) 3+

Q: What are the names of the ions Ba2+, Sn2+, and Se2-? A) barium, tin, and selenium B) barium, tin(II), and selenide C) barium(II), tin(II), and selenium(II-) D) barous, stannous, and selenide

Q: Which element can form more than one kind of monatomic ion? A) S B) Se C) Sn D) Sr

Q: Which element can form more than one kind of monatomic ion? A) Ca B) Cl C) Cr D) Cs

Q: What is the most likely charge on an ion of phosphorus, P? A) 5- B) 3- C) 3+ D) 5+

Q: Which ionic compound would be expected to have the highest lattice energy? A) Li2O B) Na2O2 C) KO2 D) RbO2

Q: Which ionic compound would be expected to have the highest lattice energy? A) NaCl B) MgO C) AlF3 D) Al2O3

Q: Which ionic compound would be expected to have the highest lattice energy? A) Na2O B) MgO C) Al2O3 D) CO2

Q: Which of the following ionic compounds would be expected to have the highest lattice energy? A) LiCl B) NaCl C) KCl D) RbCl

Q: Which of the following ionic compounds would be expected to have the highest lattice energy? A) NaF B) NaCl C) NaBr D) NaI

Q: Which chemical process is associated with the lattice energy for sodium chloride?A) NaCl(s) -> Na+(g) + Cl-(g)B) NaCl(g) -> Na+(g) + Cl-(g)C) Na(s) + 1/2 Cl2(g) -> NaCl(s)D) NaCl(s) + H2O(l) -> Na+(aq) + Cl-(aq)

Q: Calculate the electron affinity for the formation of the hydride ion from the following information: A) -50.1 kJ/mol B) -70.1 kJ/mol C) -816 kJ/mol D) -1632 kJ/mol

Q: Calculate the energy change for the formation of MgBr2(s) from its elements in their standard states: A) -150.8 kJ/mol B) -286.0 kJ/mol C) -499.2 kJ/mol D) -5682 kJ/mol

Q: Calculate the energy change in kJ/mol for the reaction using the following information:Li(g) -> Li+(g) + e- +520 kJ/molF(g) + e- -> F-(g) -328 kJ/molA) -848 kJ/molB) -192 kJ/molC) +192 kJ/molD) +848 kJ/mol

Q: Calculate the lattice energy for MgO(s) using a Born-Haber cycle and the following information: A) +1842 kJ/mol B) +2444 kJ/mol C) +3844 kJ/mol D) +4108 kJ/mol

Q: Calculate the energy change for the formation of CaF2(s) from its elements in their standard states and the following information: A) +4046 kJ/mol B) -965 kJ/mol C) -1214 kJ/mol D) -3286 kJ/mol

Q: Calculate the lattice energy for MgCl2(s) using a Born-Haber cycle and the following information: A) +641.6 kJ/mol B) +1240.5 kJ/mol C) +1882.1 kJ/mol D) +2523.7 kJ/mol

Q: Calculate the lattice energy for NaCl(s) using a Born-Haber cycle and the following information: A) +34.8 kJ/mol B) +690.3 kJ/mol C) +787.2 kJ/mol D) +1512 kJ/mol

Q: Compared to sulfur, chlorine has a ________ effective nuclear charge, Zeff, and a ________ atomic radius.

Q: Using shorthand notation, the electron configuration of Ni is ________.

Q: Copper has the anomalous electron configuration ________.

Q: According to the Bohr model of the atom, when an electron goes from a higher-energy orbit to a lower-energy orbit, it ________ electromagnetic energy with an energy that is equal to the ________ between the two orbits.

Q: An orbital with n = 4 and l = 1 is a ________ orbital.

Q: The energy of an electron in a multielectron atom depends on the quantum numbers ________ and ________.

Q: A solution to the Schrdinger wave equation is a ________, or orbital, represented by the symbol , and the probability of finding an electron defined by within a given volume of space around the nucleus is ________.

Q: Light behaves as if it were a stream of small particles, called ________, each having an amount of energy called a ________.

Q: The visible region of the electromagnetic radiation spectrum extends from ________ nm to ________ nm.

Q: Compared to ultraviolet radiation, infrared radiation occurs at ________ wavelengths, ________ frequencies, and ________ energies.

Q: Which atom in each group (I and II) has the smallest atomic radius?(I) Ba, Hf, Bi (II) As, Sb, BiA) Ba; AsB) Ba; BiC) Bi; AsD) Hf; Bi

Q: Of the following, which atom has the smallest atomic radius? A) K B) As C) Rb D) Sb

Q: Of the following, which atom has the largest atomic radius? A) Rb B) I C) Cs D) At

Q: How many valence electrons does a neutral polonium atom have? A) 2 B) 4 C) 6 D) 84

Q: Which element has the ground-state electron configuration [Xe]6s2 4f7? A) Re B) Ir C) Eu D) Gd

Q: Which of the following have the same number of valence electrons? A) Rb, Sb, I B) Ga, Sn, Bi C) As, Sb, Bi D) Ar, Kr, Br

Q: Which of the following have their valence electrons in the same shell? A) Li, N, F B) B, Si, As C) N, As, Bi D) He, Ne, F

Q: Which has the highest Zeff for its valence electrons? A) Li B) Na C) C D) F

Q: For a hydrogen atom, which electronic transition would result in the emission of a photon with the highest energy?A) 2s -> 3pB) 2p -> 6dC) 6p -> 4sD) 7f -> 5d

Q: How many orbitals are there in the fourth shell? A) 3 B) 4 C) 6 D) 16

Q: What are the possible values of l if n = 6? A) 6 B) 0, 1, 2, 3, 4, or 5 C) -4, -3, -2, -1, 0, +1, +2, +3, or +4 D) -5, -4, -3, -2, -1, 0, +1, +2, +3, +4, or +5

Q: How many subshells are there in the shell with n = 4? A) 3 B) 4 C) 6 D) 18