Chemistry & Chemical Reactivity
9th Edition
ISBN: 9781133949640
Author: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: Cengage Learning
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Textbook Question
Chapter 7.6, Problem 8Q
Use the atomic radii of scandium, yttrium, lanthanum, and lutetium to answer the questions below.
- a. Explain why lutetium has a smaller atomic radius than lanthanum, even though it has a greater number of electrons.
- b. Do the atomic radii argue for the placement of La or Lu below Y in the periodic table? Explain.
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8.Pick four elements in the main group (representative element) of the fourth period.
a.Write its abbreviated electron configuration.
b.Write the correct formula for its oxide. If it forms more than one oxide, you may list them all, but it is not necessary. If it does not form an oxide, state that.
c.Is the most common ion the element forms larger or smaller than its neutral atom? Explain your answer in terms of electronic shells/subshells.
What is the Pauli Exclusion Principle? *
a. An atomic orbital can only hold a maximum of 2 electrons, each with opposite spins
b. An atomic orbital can hold a minimum of 6 electrons, each with opposite spins
c. An atomic orbital can hold a maximum of 6 electrons, each with the same spin
d. An atomic orbital can hold a minimum of 2 electrons, each with opposite spins
Na
1.66
Compare periodic trends in atomic radii across a period (row on the periodic
table).
Li Be B C N
1.28 0.96 0.84 0.76
The atomic radii of the Period 2 elements and the Period 3 elements are shown
below.
O
0.66
Mg
0.71
Al Si P
1.41 1.21 1.11 1.07 1.05
S
F
0.57
Question 1.a of 13
Define the trend for atomic radii in a period.
Ne
0,58
Ar
CI
1.02 1.06
MacBook Air
A) atomic radii increase from the top to the
bottom down a group
B) atomic radii decrease from the top to the
bottom down a group
C) atomic radii increase from the left to right
across a period
D) atomic radii decrease from left to right
across a period
Chapter 7 Solutions
Chemistry & Chemical Reactivity
Ch. 7.1 - How many electrons can be accommodated in the n =...Ch. 7.1 - Prob. 2RCCh. 7.2 - Based on the Aufbau principle and the n + rule,...Ch. 7.3 - (a) What element has the configuration...Ch. 7.3 - Write one possible set of quantum numbers for the...Ch. 7.3 - Using the periodic table and without looking at...Ch. 7.3 - 1. What is the electron configuration of selenium...Ch. 7.3 - 2. Based on electron configurations, which of the...Ch. 7.4 - Prob. 1CYUCh. 7.4 - Prob. 1RC
Ch. 7.4 - Prob. 2RCCh. 7.4 - Which of the following species is most...Ch. 7.5 - Without looking at the figures for the periodic...Ch. 7.5 - What is the trend in sizes of the ions K+, S2, and...Ch. 7.5 - Prob. 2RCCh. 7.6 - Give the electron configurations for iron and the...Ch. 7.6 - Prob. 2QCh. 7.6 - Prob. 3QCh. 7.6 - Prob. 4QCh. 7.6 - Prob. 1RCCh. 7.6 - Prob. 2RCCh. 7.6 - The most common oxidation state of a rare earth...Ch. 7.6 - Prob. 6QCh. 7.6 - Prob. 7QCh. 7.6 - Use the atomic radii of scandium, yttrium,...Ch. 7.6 - Prob. 9QCh. 7.6 - Prob. 10QCh. 7 - Write the electron configurations for P and CI...Ch. 7 - Write the electron configurations for Mg and Ar...Ch. 7 - Using spdf notation, write the electron...Ch. 7 - Using spdf notation, give the electron...Ch. 7 - Prob. 5PSCh. 7 - Prob. 6PSCh. 7 - Use noble gas and spdf notations to depict...Ch. 7 - The lanthanides, once called the rare earth...Ch. 7 - Prob. 9PSCh. 7 - Prob. 10PSCh. 7 - What is the maximum number of electrons that can...Ch. 7 - What is the maximum number of electrons that can...Ch. 7 - Depict the electron configuration for magnesium...Ch. 7 - Depict the electron configuration for phosphorus...Ch. 7 - Using an orbital box diagram and noble gas...Ch. 7 - Using an orbital box diagram and noble gas...Ch. 7 - Using orbital box diagrams, depict an electron...Ch. 7 - Prob. 18PSCh. 7 - Prob. 19PSCh. 7 - Using orbital box diagrams and noble gas notation,...Ch. 7 - Manganese is found as MnO2 in deep ocean deposits....Ch. 7 - One compound found in alkaline batteries is NiOOH,...Ch. 7 - Prob. 23PSCh. 7 - Arrange the following elements in order of...Ch. 7 - Prob. 25PSCh. 7 - Prob. 26PSCh. 7 - Which of the following groups of elements is...Ch. 7 - Arrange the following atoms in order of increasing...Ch. 7 - Compare the elements Na, Mg, O, and P. (a) Which...Ch. 7 - Compare the elements B. Al, C, and Si. (a) Which...Ch. 7 - Explain each answer briefly. (a) Place the...Ch. 7 - Explain each answer briefly. (a) Rank the...Ch. 7 - Identify the element that corresponds to each of...Ch. 7 - Identify the element that corresponds to each of...Ch. 7 - Explain why the photoelectron spectra of hydrogen...Ch. 7 - Sketch the major features (number of peaks and...Ch. 7 - These questions are not designated as to type or...Ch. 7 - The deep blue color of sapphires comes from the...Ch. 7 - Using an orbital box diagram and noble gas...Ch. 7 - Prob. 40GQCh. 7 - Prob. 41GQCh. 7 - Prob. 42GQCh. 7 - Which of the following is not an allowable set of...Ch. 7 - A possible excited state for the H atom has an...Ch. 7 - The magnet in the following photo is made from...Ch. 7 - Name the element corresponding to each...Ch. 7 - Arrange the following atoms in order of increasing...Ch. 7 - Prob. 48GQCh. 7 - Answer the questions below about the elements A...Ch. 7 - Answer (he following questions about the elements...Ch. 7 - Which of the following ions are unlikely to be...Ch. 7 - Prob. 52GQCh. 7 - Answer each of the following questions: (a) Of the...Ch. 7 - Prob. 54GQCh. 7 - Prob. 55GQCh. 7 - Two elements in the second transition series (Y...Ch. 7 - Prob. 57GQCh. 7 - The configuration of an element is given here. (a)...Ch. 7 - Answer the questions below about the elements A...Ch. 7 - Answer the questions below concerning ground state...Ch. 7 - Nickel(II) formate [Ni(HCO2)2] is widely used as a...Ch. 7 - Spinets are solids with the general formula M2+...Ch. 7 - The following questions use concepts from this and...Ch. 7 - Which ions in the following list are not likely to...Ch. 7 - Answer the following questions about first...Ch. 7 - The ionization of the hydrogen atom can be...Ch. 7 - Compare the configurations below with two...Ch. 7 - Prob. 68SCQCh. 7 - Write electron configurations to show the first...Ch. 7 - Prob. 70SCQCh. 7 - (a) Explain why the sizes of atoms change when...Ch. 7 - Which of the following elements has the greatest...Ch. 7 - Prob. 73SCQCh. 7 - Prob. 74SCQCh. 7 - The energies of the orbitals in many elements have...Ch. 7 - The ionization energies for the removal of the...Ch. 7 - Using your knowledge of the trends in element...Ch. 7 - Prob. 78SCQCh. 7 - Prob. 79SCQCh. 7 - Prob. 80SCQCh. 7 - Thionyl chloride. SOCl2, is an important...Ch. 7 - Prob. 82SCQCh. 7 - Slaters rules are a way to estimate the effective...
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- What is the electron configuration of Mg2+? How does its reactivity compare with neutral Mg? How do the reactivities of F- and F compare?arrow_forwardExplain why Al is a member of group 13 rather than group 3?arrow_forward4. Consider the first four ionization energies for an element we will call A. Ionization energy in kJ/mol 1st 2nd 3rd 4th 578 1817 2745 11580 a. In which group does A appear on the periodic table? b. What is the most likely oxidation number for element A? c. What is the minimum number of electrons that A must have? d. Write the valence electron sublevel configuration for this element. (sublevel and number of electrons in them)arrow_forward
- 1. Calculate the effective nuclear charge of the 59th electron in Platinum 2. Give the noble gas electron configuration of Uranium 3. Give the noble gas configuration of Bromiumarrow_forwardConsider the elements: Na, Mg, Al, Si, P.a. Which element has the highest second ionization energy?b. Which element has the smallest atomic radius?c. Which element is least metallic?d. Which element is diamagnetic?arrow_forward4. Consider this chemical equation: Br + e > Br + energy Which concept does this chemical equation correspond with? A. atomic radius B. ionization energy C. electron affinity D. electronegativity E, metal reactivityarrow_forward
- 25. The photoelectric effect can be used to find which property? a. Electron Affinity b. Reactivity C. lonization Energy d. Atomic Radius 26. What charge will S have as in ion? 27. Order the following elements from most to least reactive. Mg, Si, O, Ne, K 28. Which is a true statement about solid nonmetals? a. They have a shiny and lustrous surface b. They conduct electricity and heat C. They are magnetic and ductile d. They are non-conductive, brittle, and non-ductile 29. Which statement best describes a valence electron. a. The electrons found close to the nucleus b. The electrons that are found in the outermost shell of the atom c. The total number of electrons d. Electrons that are not involved in chemical properties M SAMSUNGarrow_forwardExplain why the ionization energy of sodium (Na) is less than the ionization energy of lithium (Li). In your explanation discuss the atoms' structure: energy levels (rings), protons, and/or valence electrons.arrow_forwardConsider these elements: P, Ca, Si, S, Ga.a. Write the electron configuration for each element.b. Arrange the elements in order of decreasing atomic radius.c. Arrange the elements in order of increasing ionization energy.d. Use the electron configurations in part a to explain the differences between your answers to parts b and c.arrow_forward
- Compare Na, Mg, O and P. Which has largest atomic radius? Which has the highest ionization energy? Which has the highest metallic properties?arrow_forwardMake your own periodic table using the hypothetical elements that are given in the clues .Explain the words that will be formed if you arranged the symbols of elements correctlyarrow_forward22. Use your knowledge of electron configurations to explain why silver tends to form ions with a charge of 1+, but the element to the right of silver in the periodic table tends to form ions with a 2+ charge.arrow_forward
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