Chem 1 chapter 8 p2 and chapter 9 p1
Which of the following series of isoelectronic ions correctly lists the ions in order of increasing size (i.e., smallest to largest)? A) Ca²⁺ < K⁺ < Cl⁻ < P³⁻ B) K⁺ < Ca²⁺ < P³⁻ < Cl⁻ C) P³⁻ < Cl⁻ < K⁺ < Ca²⁺ D) Cl⁻ < K⁺ < Ca²⁺ < P³⁻ E) K⁺ < Ca²⁺ < Cl⁻ < P³⁻
A) Ca²⁺ < K⁺ < Cl⁻ < P³⁻
Which of the following is an example of an ionic bond? A) K - F B) C - H C) Kr - H D) C - F
A) K - F
In each pair, choose the atom or ion which has the appropriate property based on its position in the Periodic Table. Highest ionization energy A) Rb⁺ B) Sr⁺ Greatest electron affinity A) Xe B) I Smallest size A) Cs⁺ B) Ba²⁺
A) Rb⁺ Rb⁺ would need to lose an inner shell electron, so its ionization energy would be larger. B) I Electron affinity increases as you move from left to right on the Periodic Table, excluding the noble gases which do not want to gain electrons. B) Ba²⁺ For an isoelectronic series, the greater the positive charge, the smaller the ion is.
Which of the following oxides is expected to form the most basic aqueous solution? A) Rb₂O B) In₂O₃ C) Al₂O₃ D) SnO₂ E) TeO₂
A) Rb₂O Rb is expected to form a basic oxide because it is on the left side of the periodic table.
A lattice formation enthalpy (lattice energy) is A) the amount of energy released when individual gaseous ions combine to form an ionic solid. B) the energy released in the formation of a chemical bond. C) the difference in ionization energy and electron affinity of the anion and cation. D) the energy required to convert a substance from a solid to a gaseous state.
A) the amount of energy released when individual gaseous ions combine to form an ionic solid.
Which of the following radii comparisons is incorrect? A) Sr²⁺ < Sr B) Br⁻ < Br C) Fe³⁺ < Fe²⁺ D) Se²⁻ > Se E) Sn²⁺ > Sn⁴⁺
B) Br⁻ < Br Cations are always smaller than the neutral atom from which it is derived. Anions are always larger than the neutral atom from which it is derived.
The energy released in the reaction F(g) + e⁻ → F⁻(g) is known as the A) Ionization energy B) Electron affinity C) Enthalpy of ionization D) Electronegativity E) Enthalpy of electronegativity
B) Electron affinity The electron affinity is the change in energy when an electron is added to a neutral gaseous atom to form an ion.
Rank the following atoms in order of decreasing first ionization energies (i.e., highest to lowest): Li, Be, Ba, F. A) Ba > Li > Be > F B) F > Be > Li > Ba C) Li > Be > F > Ba D) F > Be > Ba > Li E) Ba > F > Be > Li
B) F > Be > Li > Ba In general, first ionization energy decreases down a group and increases across a period.
Choose the property that best predicts metallic behavior of elements in the periodic table. A) high ionization energy B) low ionization energy C) high electron affinity D) low electron affinity
B) low ionization energy
A lattice dissociation enthalpy (lattice energy) is A) the energy required to break a chemical bond. B) the amount of energy that must be supplied to break an ionic solid into its individual gaseous ions. C) the difference in ionization energy and electron affinity of the anion and cation. D) the energy required to convert a substance from a solid to a gaseous state.
B) the amount of energy that must be supplied to break an ionic solid into its individual gaseous ions.
Where on the periodic table would you expect to find the most acidic elemental oxides? A) Upper left corner B) Upper right corner, including noble gases C) Upper right corner, excluding noble gases D) Lower left corner E) Lower right corner, including noble gases
C) Upper right corner, excluding noble gases The upper right corner of the periodic table excluding noble gases would form the most acidic elemental oxides.
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 ionizations require the same amount of energy. C) The amount of energy required 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.
Which of the following series of isoelectronic ions (Mg²⁺, N³⁻, F⁻, Si⁴⁺) has the ionic radii in order of largest to smallest? A) Mg²⁺ > N³⁻ > F⁻ > Si⁴⁺ B) Mg²⁺ > Si⁴⁺ > F⁻ > N³⁻ C) N³⁻ > F⁻ > Si⁴⁺ > Mg²⁺ D) N³⁻ > F⁻ > Mg²⁺ > Si⁴⁺ E) F⁻ > N³⁻ > Si⁴⁺ > Mg²⁺
D) N³⁻ > F⁻ > Mg²⁺ > Si⁴⁺ For isoelectronic species, anions will be larger than cations. Ions can be further ranked by considering their charges. The greater the negative charge, the larger the size. The greater the positive charge, the smaller the size.
Which of the following elements has the smallest first ionization energy? A) S B) O C) Si D) Sr E) Cs
E) Cs Ionization energy increases from left to right and from the bottom to the top of the periodic table. Cs is the furthest to the left and closest to the bottom of the periodic table on this list. It would be predicted to have the smallest first ionization energy.
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)
