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introductory chemistry concepts

Introductory Chemistry Concepts And Critical Thinking 7th Edition Charles Corwin - Solutions

Refer to the periodic table and predict which of the following ions are isoelectronic with the noble gas xenon:(a) Cs+(b) Cl–(c) La3+(d) Se2–.Periodic Table: 2 3 4 15 6 7 3 11 Li 6.94 1 IA Na 22.99 19 37 Rb R 4 87 2 IIA Be 9.01 12 Mg 24.31 K Ca Sc 39.10 40.08 44.96 20 38 21 3 IIIB Sr Y 85.47
What is the term for the elements in the series that follows element 57?
Refer to the periodic table and write the predicted electron configuration for each of the following ions using core notation:(a) Fe3+ (b) Se2–. 2 3 4 5 6 7 Li 6.94 11 1 IA Na 22.99 19 37 55 4 2 IIA 87 Be 9.01 12 K Ca 39.10 40.08 Mg 24.31 20 38 21 Rb Sr Y 85.47 87.62 88.91 88 Sc 44.96 3 4 IIIB
Predict the next ion in the isoelectronic series: Se2–, Br–, Kr, Rb+, Sr2+.
Refer to the periodic table and write the predicted electron configuration for each of the following ions using core notation:(a) Cd2+ (b) P3–.Periodic Table: 2 3 4 15 6 7 3 11 Li 6.94 1 IA Na 22.99 19 37 Rb R 4 87 2 IIA Be 9.01 12 Mg 24.31 K Ca Sc 39.10 40.08
What is the term for the elements in the series that follows element 89?
Given the chemical formulas for Al2O3, SiO2, and P2O5, predict the formula for arsenic oxide, As?O?.
What is the electron configuration for radon gas using core notation?
What is the term for the series of elements that include Ce–Lu?
What type of elements (metal, nonmetal) are on the left side of the periodic table?Periodic Table: 2 3 4 10 6 3 7 11 Li 6.94 1 IA Na 22.99 19 37 5 Rb K 39.10 al 55 4 87 2 IIA Fr (223) Be 9.01 12 Mg 24.31 Sr 85.47 87.62 20 38 Ca Sc 40.08 44.96 21 56 Cs La Ba 132.91 137.33
Can ions of different elements have the same number of electrons?
What is the term for the series of elements that include Th–Lr?
Can ions of different elements have the same number of protons?
What type of elements (metal, nonmetal) are on the right side of the periodic table?Periodic Table: 2 3 4 10 6 3 7 11 Li 6.94 1 IA Na 22.99 19 37 5 Rb K 39.10 al 55 4 87 2 IIA Fr (223) Be 9.01 12 Mg 24.31 Sr 85.47 87.62 20 38 Ca Sc 40.08 44.96 21 56 Cs La Ba 132.91 137.33
Can ions of different elements have the same number of neutrons?
The following photograph shows a semimetal (Sb), nonmetal (S), and compound, (Sb2S5). Identify the (a) Yellow, (b) Gray,(c) Orange substances.
Which two elements are rare earth elements, but not lanthanides?
Which two elements are radioactive semimetals?
Identify the group number corresponding to each of the following families of elements.(a) Alkali metals (b) Alkaline earth metals (c) Halogens (d) Noble gases.
Refer to the periodic table and select the symbol of the element that fits each of the following descriptions.(a) The semimetal in the second period (b) The semimetal in the fourth period and Group IVA/14 (c) The halogen that exists as yellow gas (d) The halogen that is radioactive.Periodic
Identify the group number corresponding to each of the following families of elements.(a) Boron group (b) Oxygen group (c) Nickel group (d) Copper group.
Refer to the periodic table and select the symbol of the element that fits each of the following descriptions.(a) The third–period alkali metal (b) The third–period alkaline earth metal (c) The rare earth element with the highest atomic mass (d) The lanthanide that is radioactive.Periodic
Refer to the periodic table and select the symbol of the element that fits each of the following descriptions.(a) The semimetal in the third period (b) The semimetal in the fourth period and Group VA/15 (c) The halogen that exists as a reddish-brown liquid (d) The noble gas that is
According to IUPAC convention, what is the designation for each of the following groups of elements?(a) Group IA (b) Group IIIA (c) Group VA (d) Group VIIA (e) Group IB (f) Group IIIB (g) Group VB (h) Group VIIB.
According to the American convention, what is the designation for each of the following groups of elements?(a) Group 2 (b) Group 4 (c) Group 6 (d) Group 8 (e) Group 11 (f) Group 12 (g) Group 16 (h) Group 18.
Refer to the periodic table and select the symbol of the element that fits each of the following descriptions.(a) The fourth–period alkali metal (b) The fourth–period alkaline earth metal (c) The rare earth element with the lowest atomic mass (d) The lanthanide that does not occur
According to the general trend, metallic character (increases/decreases) proceeding up a group of elements in the periodic table.Periodic Table: 2 3 4 10 6 3 7 11 Li 6.94 1 IA Na 22.99 19 37 5 Rb K 39.10 al 55 4 87 2 IIA Fr (223) Be 9.01 12 Mg 24.31 Sr 85.47 87.62 20 38 Ca Sc 40.08
According to the general trend, metallic character (increases/decreases) proceeding from left to right in the periodic table.Periodic Table: 2 3 4 10 6 3 7 11 Li 6.94 1 IA Na 22.99 19 37 5 Rb K 39.10 al 55 4 87 2 IIA Fr (223) Be 9.01 12 Mg 24.31 Sr 85.47 87.62 20 38 Ca Sc 40.08
According to the general trend, the atomic radius (increases/decreases) proceeding up a group of elements in the periodic table.Periodic Table: 2 3 4 10 6 3 7 11 Li 6.94 1 IA Na 22.99 19 37 5 Rb K 39.10 al 55 4 87 2 IIA Fr (223) Be 9.01 12 Mg 24.31 Sr 85.47 87.62 20 38 Ca Sc 40.08
According to the general trend, the atomic radius (increases/decreases) proceeding from left to right in the periodic table.Periodic Table: 2 3 4 10 6 3 7 11 Li 6.94 1 IA Na 22.99 19 37 5 Rb K 39.10 al 55 4 87 2 IIA Fr (223) Be 9.01 12 Mg 24.31 Sr 85.47 87.62 20 38 Ca Sc 40.08
According to general trends in the periodic table, predict which element in each of the following pairs has the greater metallic character.(a) K or Ca (b) Mg or Al (c) Fe or Cu (d) S or Ar.Periodic Table: 2 3 4 10 6 3 7 11 Li 6.94 1 IA Na 22.99 19 37 5
According to general trends in the periodic table, predict which element in each of the following pairs has the greater metallic character.(a) B or Al (b) Na or K (c) Mg or Ba (d) H or Fe.Periodic Table: 2 3 4 10 6 3 7 11 Li 6.94 1 IA Na 22.99 19 37 5
According to general trends in the periodic table, predict which element in each of the following pairs has the larger atomic radius.(a) Li or Na (b) N or P (c) Mg or Ca (d) Ar or Kr.Periodic Table: 2 3 4 10 6 3 7 11 Li 6.94 1 IA Na 22.99 19 37 5
According to general trends in the periodic table, predict which element in each of the following pairs has the larger atomic radius.(a) Rb or Sr(b) As or Se (c) Pb or Bi (d) I or Xe.Periodic Table: 2 3 4 10 6 3 7 11 Li 6.94 1 IA Na 22.99 19 37 5
Predict the missing value (?) for radioactive francium (Fr). The atomic radius, density, and melting point are given for elements in Group IA/1. Element Atomic Radius 248 pm 266 pm (?) pm Rb Cs Fr Density at 20°C 1.53 g/mL 1.93 g/mL (?) g/mL Melting Point 39.3 °C 28.4 °C (?) °C
The formulas for the chlorides of potassium, calcium, boron, and germanium are, respectively, KCl, CaCl2, BCl3, and GeCl4. Using the periodic table, predict the chemical formulas for each of the following similar compounds.(a) Potassium fluoride (b) Calcium fluoride (c) Boron bromide (d)
Predict the missing value (?) for radioactive radium (Ra). The atomic radius, density, and melting point are given for elements in Group IIA/2. Element Atomic Radius 215 pm 217 pm (?) pm Sr Ba Ra Density at 20 Density at 20 °C °C 2.63 g/mL 3.65 g/mL (?) g/mL Melting Point 769 °C 725 °C (?) °C
The formulas for the oxides of sodium, magnesium, aluminum, and silicon are, respectively, Na2O, MgO, Al2O3, and SiO2. Using the periodic table, predict the chemical formulas for each of the following similar compounds.(a) Lithium oxide (b) Barium oxide (c) Gallium oxide (d) Tin oxide.Periodic
Predict the missing value (?) for radioactive astatine (At). The atomic radius, density, and boiling point are given for elements in Group VIIIA/17. Element Br I At Atomic Radius 115 pm 133 pm (?) pm Density at 20 °C Density at 20 °C 3.10 g/L 4.93 g/L (?) g/L Boiling Point 59 °C 184 °C (?) °C
Predict the missing value (?) for radioactive radon (Rn). The atomic radius, density, and boiling point are given for elements in Group VIIIA/18. Element Kr Xe Rn Atomic Radius 202 pm 210 pm (?) pm Density at STP 3.74 g/L 5.86 g/L (?) g/L Boiling Point -152 °C -107 °C (?) °C
The chemical formula for barium chloride is BaCl2. Predict the formulas for each of the following similar compounds.(a) Calcium fluoride (b) Calcium chloride (c) Calcium bromide (d) Calcium iodide.
The chemical formula for zinc oxide is ZnO. Predict the formulas for each of the following similar compounds.(a) Cadmium oxide (b) Cadmium sulfide (c) Cadmium selenide (d) Cadmium telluride.
Depending upon reaction conditions, nitrogen and oxygen can produce either N2O3 or N2O5. Predict two formulas for each of the following compounds.(a) Arsenic oxide (b) Antimony oxide.
Depending upon reaction conditions, phosphorus and sulfur can produce either P2S3 or P2S5. Predict two formulas for each of the following compounds.(a) Arsenic sulfide (b) Antimony sulfide.
What type of energy sublevel (s, p, d, f) is being filled by the elements in Groups IA/1 and IIA/2?
What type of energy sublevel (s, p, d, f) is being filled by the elements in Groups IIIA/13 through VIIIA/18?
Refer to the periodic table and state the highest energy sublevel for each of the following elements.(a) H (b) Na (c) Sm (d) Br (e) Sr (f) C (g) Sn (h) Cs.Periodic Table: 2 3 4 10 6 3 7 11 Li 6.94 1 IA Na 22.99 19 37 5 Rb K 39.10 al 55 4 87 2 IIA Fr (223) Be 9.01 12 Mg 24.31 Sr 85.47
What type of energy sublevel (s, p, d, f) is being filled by the transition elements?
Refer to the periodic table and state the highest energy sublevel for each of the following elements.(a) He (b) K (c) U (d) Pd (e) Be (f) Co (g) Si (h) Pt.Periodic Table: 2 3 4 10 6 3 7 11 Li 6.94 1 IA Na 22.99 19 37 5 Rb K 39.10 al 55 4 87 2 IIA Fr (223) Be 9.01 12 Mg 24.31 Sr 85.47
What type of energy sublevel (s, p, d, f) is being filled by the inner transition elements?
Refer to the periodic table and write the predicted electron configuration for each of the following elements.(a) Li (b) F (c) Mg (d) P (e) Ca (f) Mn (g) Ga (h) Rb.Periodic Table: 2 3 4 10 6 3 7 11 Li 6.94 1 IA Na 22.99 19 37 5
Which energy sublevel is being filled by the lanthanide series?
Refer to the periodic table and write the predicted electron configuration for each of the following elements.(a) B (b) Ti (c) Na (d) O (e) Ge (f) Ba (g) Pd (h) Kr.Periodic Table: 2 3 4 10 6 3 7 11 Li 6.94 1 IA Na 22.99 19 37 5
Which energy sublevel is being filled by the actinide series?
State the number of valence electrons in each of the following groups as predicted from the periodic table.(a) Group IIA/2 (b) Group IVA/14 (c) Group VIA/16 (d) Group VIIIA/18.Periodic Table: 2 3 4 10 6 3 7 11 Li 6.94 1 IA Na 22.99 19 37 5
According to the general trend, the ionization energy for a group of elements (increases/decreases) proceeding up a group in the periodic table.Periodic Table: 2 3 4 10 6 3 7 11 Li 6.94 1 IA Na 22.99 19 37 5 Rb K 39.10 al 55 4 87 2 IIA Fr (223) Be 9.01 12 Mg 24.31 Sr 85.47 87.62 20 38 Ca Sc 40.08
State the number of valence electrons for each of the following elements.(a) H (b) B (c) N (d) F (e) Ca (f) Si (g) O (h) Ar.
According to the general trend, the ionization energy for a period of elements (increases/decreases) proceeding from left to right in the periodic table.Periodic Table: 2 3 4 10 6 3 7 11 Li 6.94 1 IA Na 22.99 19 37 5 Rb K 39.10 al 55 4 87 2 IIA Fr (223) Be 9.01 12 Mg 24.31 Sr 85.47
State the number of valence electrons for each of the following elements.(a) He (b) Pb (c) Se (d) Ne (e) Cs (f) Ga (g) Sb (h) Br.
Draw the electron dot formula for each of the following elements.(a) H (b) B (c) N (d) F (e) Ca (f) Si (g) O (h) Ar.
Draw the electron dot formula for each of the following elements.(a) He (b) Pb (c) Se (d) Ne (e) Cs (f) Ga (g) Sb (h) Br.
Refer to the periodic table and predict which element in each of the following pairs has the higher ionization energy.(a) Mg or Ca (b) S or Se (c) Sn or Pb (d) N or P.Periodic Table: 2 3 4 10 6 3 7 11 Li 6.94 1 IA Na 22.99 19 37 5 Rb K 39.10 al 55 4 87 2 IIA Fr (223) Be 9.01 12 Mg 24.31 Sr 85.47
Refer to the periodic table and predict which element in each of the following pairs has the higher ionization energy.(a) Ga or Ge (b) Si or P(c) Br or Cl (d) As or Sb.Periodic Table: 2 3 4 10 6 3 7 11 Li 6.94 1 IA Na 22.99 19 37 5 Rb K 39.10 al 55 4 87 2 IIA Fr (223) Be 9.01 12 Mg 24.31 Sr 85.47
Refer to the periodic table and predict which element in each of the following pairs has the lower ionization energy.(a) Rb or Cs (b) He or Ar (c) B or Al (d) F or I.Periodic Table: 2 3 4 10 6 3 7 11 Li 6.94 1 IA Na 22.99 19 37 5 Rb K 39.10 al 55 4 87 2 IIA Fr (223) Be 9.01 12 Mg 24.31 Sr 85.47
Which group of elements has the lowest ionization energy?
Which group of elements has the highest ionization energy?
State the number of valence electrons in each of the following groups as predicted from the periodic table.(a) Group IA/1 (b) Group IIIA/13 (c) Group VA/15 (d) Group VIIA/17.Periodic Table: 2 3 4 10 6 3 7 11 Li 6.94 1 IA Na 22.99 19 37 5
Refer to the periodic table and predict which element in each of the following pairs has the lower ionization energy.(a) Mg or Si(b) Pb or Bi (c) Ca or Ga (d) P or Cl.Periodic Table: 2 3 4 10 6 3 7 11 Li 6.94 1 IA Na 22.99 19 37 5 Rb K 39.10 al 55 4 87 2 IIA Fr (223) Be 9.01 12 Mg 24.31 Sr 85.47
State the predicted ionic charge of metal ions in each of the following groups of elements.(a) Group IA/1 (b) Group IIA/2 (c) Group IIIA/13 (d) Group IVA/14.
State the predicted ionic charge of nonmetal ions in each of the following groups of elements.(a) Group IVA/14 (b) Group VA/15 (c) Group VIA/16 (d) Group VIIA/17.
Write the ionic charge for each of the following ions as predicted from the group number in the periodic table.(a) Be ion (b) Sn ion (c) P ion (d) S ion.Periodic Table: 2 3 4 10 6 3 7 11 Li 6.94 1 IA Na 22.99 19 37 5 Rb K 39.10 al 55 4 87 2 IIA Fr (223) Be 9.01 12 Mg 24.31 Sr 85.47
Write the ionic charge for each of the following ions as predicted from the group number in the periodic table.(a) Cs ion (b) Ga ion (c) O ion (d) I ion.Periodic Table: 2 3 4 10 6 3 7 11 Li 6.94 1 IA Na 22.99 19 37 5 Rb K 39.10 al 55 4 87 2 IIA Fr (223) Be 9.01 12 Mg 24.31 Sr 85.47
Refer to the periodic table and predict which of the following ions are isoelectronic with the noble gas argon.(a) Al3+ (b) Ca2+(c) S2–(d) N3–.Periodic Table: 2 3 4 10 6 3 7 11 Li 6.94 1 IA Na 22.99 19 37 5 Rb K 39.10 al 55 4 87 2 IIA Fr (223) Be 9.01 12 Mg 24.31 Sr 85.47
Refer to the periodic table and predict which of the following ions are isoelectronic with the noble gas krypton.(a) K+ (b) Sr2+(c) Cl– (d) Se2–.
Refer to the periodic table and write the predicted electron configuration for each of the following positive ions using core notation.(a) Mg2+ (b) K+(c) Fe2+ (d) Zr2+.Periodic Table: 2 3 4 10 6 3 7 11 Li 6.94 1 IA Na 22.99 19 37 5 Rb K 39.10 al 55 4 87 2 IIA Fr (223) Be 9.01 12 Mg 24.31 Sr 85.47
Refer to the periodic table and write the predicted electron configuration for each of the following positive ions using core notation.(a) Ti2+ (b) Zn2+(c) Y3+ (d) Cs+.Periodic Table: 2 3 4 10 6 3 7 11 Li 6.94 1 IA Na 22.99 19 37 5 Rb K 39.10 al 55 4 87 2 IIA Fr (223) Be 9.01 12 Mg 24.31 Sr 85.47
Refer to the periodic table and write the predicted electron configuration for each of the following negative ions using core notation.(a) F–(b) S2–(c) N3–(d) I–.Periodic Table: 2 3 4 10 6 3 7 11 Li 6.94 1 IA Na 22.99 19 37 5 Rb K 39.10 al 55 4 87 2 IIA Fr (223) Be 9.01 12 Mg 24.31 Sr 85.47
Refer to the periodic table and write the predicted electron configuration for each of the following negative ions using core notation.(a) Br–(b) Te2–(c) As3–(d) O2–.Periodic Table: 2 3 4 10 6 3 7 11 Li 6.94 1 IA Na 22.99 19 37 5
Use the American convention to designate the group number corresponding to each of the following groups listed by the European convention.(a) Group IA (b) Group IB (c) Group IIIA (d) Group IIIB.
Use the IUPAC convention to designate the group number corresponding to each of the following groups listed by the European convention.(a) Group IIA (b) Group IIB (c) Group IVA (d) Group IVB.
Predict the missing value (?) for each property listed below. The atomic radius, density, and boiling point are given for elements in Group VIB/6. Element Cr Mo W Atomic Radius 125 pm (?) pm 137 pm Density at 20 °C Melting Point (?) °C 2617 °C 3410 °C 7.14 g/mL 10.28 g/mL (?) g/mL
Predict the missing value (?) for each property listed below. The atomic radius, density, and melting point are given for elements in Group VIII/8. Element Fe Ru Os Atomic Radius 126 pm (?) pm 135 pm Density at 20 °C Melting Point 7.87 g/mL (?) °C 12.45 g/mL 2334 °C (?) g/mL 3033 °C
Refer to the periodic table and write the predicted electron configuration for each of the following elements using core notation.(a) Sr (b) Ru (c) Sb (d) Cs.Periodic Table: 2 3 4 10 6 3 7 11 Li 6.94 1 IA Na 22.99 19 37 5 Rb K 39.10 al 55 4 87 2 IIA Fr (223) Be 9.01 12 Mg 24.31 Sr 85.47
Refer to the periodic table and write the predicted electron configuration for each of the following elements using core notation.(a) W (b) Bi (c) Ra (d) Ac.Periodic Table: 2 3 4 10 6 3 7 11 Li 6.94 1 IA Na 22.99 19 37 5 Rb K 39.10 al 55 4 87 2 IIA Fr (223) Be 9.01 12 Mg 24.31 Sr 85.47
Supply a systematic name for each of the following monoatomic anions:(a) Br– (b) N3–.
Explain why the ionization energy for hydrogen is much higher than that of other Group IA/1 elements.
Predict two ionic charges for hydrogen. Write the formulas of the two ions and explain the ionic charges.
Examine Figure 5.1 and determine the name of the element that Mendeleev predicted before its discovery and called ekaboron.Figure 5.1 Group Formula of Oxide I R₂0 = 32 × 3 2 2011 21 Cu Ag Au II RO Be Mg Ca Zn Sr Cd Ba Hg III R₂O3
Examine Figure 5.1 and determine the name of the element that Mendeleev predicted before its discovery and called ekaaluminum.Figure 5.1 Group Formula of Oxide I R₂0 = = 2 × 3 2 2011 21 Cu Ag Au II RO Be Mg Ca Zn Sr Cd Ba Hg III R₂O3
Explain why the ionization energy for the alkali metals is less than the ionization energy for the alkaline earth metals.
Explain why the ionization energy for aluminum, contrary to the general trend, is less than the ionization energy for magnesium.
How do you distinguish a binary molecular compound from a binary acid?
Classify each of the following as a binary ionic compound, ternary ionic compound, binary molecular compound, binary acid, or ternary oxyacid.(a) Water, H2O (b) Rust, Fe2O3 (c) Marble, CaCO3 (d) Stomach acid, HCl(aq).
Classify each of the following as binary ionic, ternary ionic, binary molecular, binary acid, or ternary oxyacid: NaCl, HCl, HCl(aq), NaClO3, HClO3(aq).
The element actinium is unstable and radioactive. Use the periodic table to predict the formula for actinium chloride, given the formula of lanthanum chloride, LaCl3. Periodic table of the elements Alkali metals Alkaline-earth metals Transition metals Other metals Other
Write the chemical formula for the following binary compounds given their constituent ions:(a) Iron(II) sulfide, Fe2+ and S2- (b) Mercury(I) fluoride, Hg22+ and F-(c) Lead(IV) oxide, Pb4+ and O2-.
Write the chemical formula for the following binary compounds given their constituent ions:(a) Copper(I) oxide, Cu+ and O2–(b) Cadmium oxide, Cd2+ and O2–(c) Cobalt(III) oxide, Co3+ and O2–.
Provide the formula for each of the following polyatomic oxyanions:(a) Acetate ion (b) Dichromate ion (c) Perchlorate ion (d) Hydrogen carbonate ion.
Provide a systematic name for each of the following polyatomic oxyanions:(a) CO32– (b) CrO42– (c) ClO2– (d) HSO4–.
Provide the formula for each of the following monoatomic anions:(a) Fluoride ion (b) Oxide ion

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