Mastering Chapter 7
Arrange F, I-, Cl-, and Br- in order of increasing radii.
F, Cl- , Br-, I-
Use the following equation to solve this problem: Zeff=Z−S Among elements 1 to 18, which element or elements have the smallest effective nuclear charge? largest? H Li Na Be Mg B Al C Si N P O S F Cl Ne Ar
H = 1-0 = 1 Li = 3-2 = 1 Na = 11 - 10 = 1 Be = 4 - 2 = 2 Mg = 12 - 10 = 2 B = 5 - 2 = 3 Al = 13 - 10 = 3 C = 6 - 2 = 4 Si = 14 - 10 = 4 N = 7 - 2 = 5 P = 5 O = 6 S = 6 F = 7 Cl = 7 Ne = 8 Ar = 8 smallest: H, Li, Na largest: Ar, Ne
Would you expect manganese(II) oxide, MnO, to react more readily with HCl(aq) or KOH(aq)?
HCl
What is the relationship between the ionization energy of an anion with a -1 charge, such as F−, and the electron affinity of the neutral atom, F?
IE of F- = - EF of F
Which of the following correctly describes the measurement of an atom's electron affinity? It is a positive value. It measures the ease with which an atom gains an electron. It is a measure of the ease with which an atom loses an electron. It is a measurement of the energy change associated with forming a positively charged ion from a neutral atom.
It measures the ease with which an atom gains an electron.
Predict whether each of the following oxides is ionic or molecular. SnO2 CO2 H2O Fe2O3 Al2O3 Li2O
Molecular: CO2, H2O Ionic: Fe2O3, Al2O3, Li2O, SnO2
Which element has the highest second ionization energy? Al, Mg, Rb, Na
Na
Rank the following items in order of decreasing radius: Na, Na+, and Na−.
Na-, Na, Na+
If the electron affinity for an element is a negative number, does it mean that the anion of the element is more stable than the neutral atom? No, it means that the cation of the element is more stable than the neutral atom. Yes, the anion is lower in energy than a neutral atom. Yes, the anion is higher in energy than a neutral atom. No, it means that an electron in an atom or ion is lower in energy than a free electron.
No, it means that an electron in an atom or ion is lower in energy than a free electron. A negative value for electron affinity implies that the added electron is more stable than a free electron. This is due to a stabilization that results from the attraction of the electron to the nucleus
Which of the following statements about the bonding atomic radii is incorrect? For a given period, the radii of the representative elements generally decrease from left to right across a period. The radii of the representative elements for the n=3 period are all larger than those of the corresponding elements in the n=2 period. The large radii of the group 1A (1) elements are due to their relatively small effective nuclear charges. For most of the representative elements, the change in radius from the n=2 to the n=3 period is greater than the change in radius from n=3 to n=4. The radii of the transition elements generally increase from left to right within a period.
The radii of the transition elements generally increase from left to right within a period.
How do cations of the same charge change in radius as you move down a column in the periodic table? They get smaller, just like the atoms do. They get smaller, inversely to the atoms do. They get larger, inversely to the atoms do. They get larger, just like the atoms do.
They get larger, just like the atoms do.
write the equation for the fourth ionization energy of zirconium
Zr+3(g) -> Zr+4(g) + e-
What is the ground state electronic configuration of Ti+4?
[Ar]
What is the ground-state electron configuration of the chloride ion Cl−?
[Ar]
What is the ground-state electron configuration of a neutral atom of manganese?
[Ar] 4s2 3d5
Write the electron configuration for As3−
[Ar]4s^2 3d^10 4p^6
Write the electron configuration for Y3+
[Ar]4s^23d^104p^6
Write electron configuration for Ru3+
[Kr]4d^5
Write the electron configuration for Pd2+
[Kr]4d^8
Write the electron configuration for Au3+
[Xe]4f^145d^8
Write the electron configuration for Pb2+
[Xe]6s^24f^145d^10
Which would you expect to experience a greater effective nuclear charge? a 2p electron of a Ne atom a 3s electron of a Na atom
a 2p electron of a Ne atom
In 1913, the English physicist Henry Moseley developed the concept of atomic numbers. He correctly identified the atomic number with which of the following? a. The atomic weight of an atom b. The number of neutrons in the nucleus of the atom c. The number of protons in the nucleus of the atom and the number of electrons in the atom d. The number of protons and neutrons in the nucleus of an atom
c
Arrange these electrons in order of decreasing effective nuclear charge: a 1s electron in carbon, a 3s electron in silicon, a 3s electron in germanium, and a 1s electron in tin. a. Ge 3s > Si 3s > Sn 1s > C 1s b. C 1s > Si 3s > Ge 3s > Sn 1s c. Sn 1s > Ge 3s > Si 3s > C 1s d. Sn 1s > Ge 3s > C 1s > Si 3s
d
Which statement is true about the effective nuclear charge (Zeff)? a The effective nuclear charge decreases from left to right across any period in the periodic table. b The effective nuclear charge increases from right to left across any period in the periodic table. c The effective nuclear charge decreases as we go down a column. d The effective nuclear charge increases as we go down a column.
d
Which of the following statements about effective nuclear charge for the outermost valence electron of an atom is incorrect? a. Effective nuclear charge increases going left to right across a row of the periodic table. b. The effective nuclear charge shows a sudden decrease when we go from the end of one row to the beginning of the next row of the periodic table c. The change in effective nuclear charge going down a column of the periodic table is generally less than that going across a row of the periodic table. d. The effective nuclear charge can be thought of as the true nuclear charge minus a screening constant due to the other electrons in the atom e. Valence electrons screen the nuclear charge more effectively than do core electrons.
e
Estimate the As−I bond length from the data As has a radius of 1.19 Å I has a radius of 1.33 Å
2.52 Å
Determine which have noble-gas configurations. Ru3+ As3− Y3+ Pd2+ Pb2+ Au3+
As3− Y3+
Rank the following ions in order of decreasing radius: F−,Cl−,Br−,I−, and At-
At-, I-, Br-, Cl-, F-
Given Ba, Li, Na, Cs, and Be, arrange the group 1 and 2 elements in order of increasing reactivity to water (H2O).
Be, Li, Ba, Na, Cs
Arrange the elements S, P, Cl, and Ca in order of increasing electronic affinity (EA).
Ca<P<S<Cl
Arrange the following oxides in order of increasing acidity. CaO CO2 SiO2 SO3 Al2O3 P2O5
CaO, Al2O3, SiO2, CO2, P2O5, SO3
Which list correctly gives atoms in order of increasing size? Cl < P < Xe < Br P < Cl < Br < Xe Cl < P < Br < Xe Xe < Br < P < Cl
Cl < P < Br < Xe
Given TeO2, Cr2O3, Cl2O, and N2O5 which oxide is expected to form a hydroxide in water?
Cr2O3 its a metal
The following ions contain the same number of electrons. Rank them in order of decreasing ionic radii. Ca2+, Cl-, S2-, K+, P3-, Sc3+
P3-, S2-, Cl-, K+, Ca2+, Sc3+
what are the equations for first two ionization energies of lead.
Pb(g) -> Pb+(g) + e- Pb+(g) -> Pb+2 (g) +e-
Which element has the following configuration: [Xe]6s24f5?
Pm
Why it is easier to remove a 2p electron from an oxygen atom than from a nitrogen atom? In the case of oxygen there are more electrons in the atom so they have to move in a higher radii orbite and can easier separate. There is more electron-electron repulsion in the case of oxygen because two electrons have to occupy the same orbital. It is easier to remove a 2p electron from an oxygen atom because oxygen is more electronegative than nitrogen. In the oxygen atom the nucleus is much smaller so attraction between it and electrons is lower.
There is more electron-electron repulsion in the case of oxygen because two electrons have to occupy the same orbital.
Which is not a characteristic of metals? They are poor conductors of heat and electricity. They have a shiny luster and various colors, although most are silvery. Most metal oxides are ionic solids that are basic. Solids are malleable and ductile.
They are poor conductors of heat and electricity.
