4. As you move across the periodic table, from left to right,(A) do the atoms get smaller or larger?(B) are the ionization energies increasing or decreasing?(C) are the metals becoming more or less reactive?

1. As we move left to right in a period, the size of atoms gets smaller. Explanation: As we move…

Answered: 4. As you move across the periodic…

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter7: Atomic Structure And Periodicity

Section: Chapter Questions

Problem 131E: Does the information on alkali metals in Table 2-8 of the text confirm the general periodic trends...

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Similar questions

Which of these isoelectronic ions, Ba2+, Cs+, or La3+, is (a) the largest? (b) the smallest? Explain your reasoning.
Despite the expected decrease in atomic size, there is an unexpected drop in IE1 values between Groups 2A(2) and 3A(13) in Periods 2 through 4. Explain this pattern in terms of electron configurations and orbital energies.
Based on the ionization energies of the alkali metals (see Section3.7), which alkali metal would you expect to undergo the most exothermic reaction with chlorine gas? Write a balanced chemical equation for the reaction.
Boron, atomic number 5, occurs naturally as two isotopes, 10B and 11B, with natural abundances of 19.9% and 80.1%, respectively.(a) In what ways do the two isotopes differ from each other? Does the electronic configuration of 10B differ from that of 11B? (b) Drawthe orbital diagram for an atom of 11B. Which electrons are the valence electrons? (c) Indicate three ways in which the 1s electrons inboron differ from its 2s electrons. (d) Elemental boron reacts with fluorine to form BF3, a gas. Write a balanced chemical equation forthe reaction of solid boron with fluorine gas. (e) ΔHf° for BF31g2 is -1135.6 kJ>mol. Calculate the standard enthalpy change in thereaction of boron with fluorine. (f) Will the mass percentage of F be the same in 10BF3 and 11BF3? If not, why is that the case?
Which elements on the periodic table tend to have the lowest first ionisation energy? What is the implication of this?
What is the maximum number of electrons in an n = 2 shell?
Boron, atomic number 5, occurs naturally as two isotopes, 10B and 11B, with natural abundances of 19.9% and 80.1%, respectively. (a) In what ways do the two isotopes differ from each other? Does the electronic configuration of 10B differ from that of 11B? (b) Draw the orbital diagram for an atom of 11B. Which electrons are the valence electrons? (c) Indicate three ways in which the 1s electrons in boron differ from its 2s electrons. (d) Elemental boron reacts with fluorine to form BF3, a gas. Write a balanced chemical equation for the reaction of solid boron with fluorine gas. (e) ΔHf° for BF3(g) is -1135.6 kj/mol. Calculate the standard enthalpy change in the reaction of boron with fluorine. (f) Will the mass percentage of F be the same in 10BF3 and 11BF3? If not, why is that the case?
Which statements completed with a to e will be true and whichwill be false?In Group 4A (14), an atom of C compared to an atom of Sn hasa larger (greater)a. atomic sizeb. ionization energyc. number of protonsd. metallic charactere. number of valence electrons
Which of these spheres represents F, which represents Br,and which represents Br-?
7.34 On the basis of their positions in the periodic table, select the atom with the larger atomic radius in each of the following pairs: (a) Na, Si; (b) Ba, Be; (c) N, F; (d) Br, Cl; (e) Ne, Kr.

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4. As you move across the periodic table, from left to right, (A) do the atoms get smaller or larger? (B) are the ionization energies increasing or decreasing? (C) are the metals becoming more or less reactive?