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4. How many electrons does sulfur have in the 3p orbital? a. 4 b. 5 C. 6 5. Which of the following molecules would NOT have resonance structures? a. CO3²- b. S03 c.NHẬ d. 0 A, B, and C It is impossible for molecules of the form AX2 to be polar 6. Which factor affects whether a molecule of the general form AX₂ is polar? a. The electronegativity difference between atoms within the molecule that are bonded to each other Whether there are lone pairs of electrons on the peripheral atoms b. C. Whether there are lone pairs of electrons on the central atom A and C d. e. f. d. 03

4. How many electrons does sulfur have in the 3p orbital? a. 4 b. 5 C. 6 5. Which of the following molecules would NOT have resonance structures? a. CO3²- b. S03 c.NHẬ d. 0 A, B, and C It is impossible for molecules of the form AX2 to be polar 6. Which factor affects whether a molecule of the general form AX₂ is polar? a. The electronegativity difference between atoms within the molecule that are bonded to each other Whether there are lone pairs of electrons on the peripheral atoms b. C. Whether there are lone pairs of electrons on the central atom A and C d. e. f. d. 03

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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4. How many electrons does sulfur have in the 3p orbital? a. 4 b. 5 5. Which of the following molecules would NOT have resonance structures? a. CO3²- b. S03 c. NHÀ 6. Which factor affects whether a molecule of the general form AX2 is polar? a. b. C. d. e. f. 7. The middle carbon in H₂CCCH₂ has what type of hybridization? a. sp² b. sp 8. Diamond is an example of: a. an ionic crystal b. a molecular crystal A, B, and C It is impossible for molecules of the form AX2 to be polar a. The electronegativity difference between atoms within the molecule that are bonded to each other Whether there are lone pairs of electrons on the peripheral atoms Whether there are lone pairs of electrons on the central atom A and C b. c. 6 9. Which molecule would be expected to have the highest boiling point? b. CCl4 a. CH4 C. CO₂ 11. A triple bond contains: 10. The electron configuration diagram shown to the right for nitrogen: is correct is incorrect because it violates Hund's rule is incorrect because it violates the Aufbau principle d. is incorrect because it violates the Pauli exclusion principle One sigma and two pi bonds One pi bond and two sigma bonds b. c. Three sp³ hybrid orbitals d. Three sigma bonds c. sp³ d. can't be determined c. P-Cl: d. Si-F: c. a metallic crystal d. a network solid 12. Classify each bond as non-polar covalent (N), polar covalent (P), or ionic (1). a. Mg-0: b. N-Br: d. 0 d. 03 H- N, O,F D- Pelop CH₂Clz 11111 1s 2s 2p (2 pts)
Transcribed Image Text:4. How many electrons does sulfur have in the 3p orbital? a. 4 b. 5 5. Which of the following molecules would NOT have resonance structures? a. CO3²- b. S03 c. NHÀ 6. Which factor affects whether a molecule of the general form AX2 is polar? a. b. C. d. e. f. 7. The middle carbon in H₂CCCH₂ has what type of hybridization? a. sp² b. sp 8. Diamond is an example of: a. an ionic crystal b. a molecular crystal A, B, and C It is impossible for molecules of the form AX2 to be polar a. The electronegativity difference between atoms within the molecule that are bonded to each other Whether there are lone pairs of electrons on the peripheral atoms Whether there are lone pairs of electrons on the central atom A and C b. c. 6 9. Which molecule would be expected to have the highest boiling point? b. CCl4 a. CH4 C. CO₂ 11. A triple bond contains: 10. The electron configuration diagram shown to the right for nitrogen: is correct is incorrect because it violates Hund's rule is incorrect because it violates the Aufbau principle d. is incorrect because it violates the Pauli exclusion principle One sigma and two pi bonds One pi bond and two sigma bonds b. c. Three sp³ hybrid orbitals d. Three sigma bonds c. sp³ d. can't be determined c. P-Cl: d. Si-F: c. a metallic crystal d. a network solid 12. Classify each bond as non-polar covalent (N), polar covalent (P), or ionic (1). a. Mg-0: b. N-Br: d. 0 d. 03 H- N, O,F D- Pelop CH₂Clz 11111 1s 2s 2p (2 pts)
1. The fact that most alpha particles passed directly through the foil in Rutherford's gold foil experiment led to the discovery that: a. the atom contains a large nucleus that takes up a majority of its space b. the atom is mostly empty space C. d. e. 2. An electron has the quantum numbers n= 3,1 2, m = 1,m, = +. In which orbital is this electron Hund's found? the atom contains electrons, which don't interact with alpha particles electrons orbit the nucleus in fixed energy level B & C a. 2p b. 3s 3. The orbital diagram to the right represents an electron configuration for: A transition metal An alkali metal An alkaline earth metal A lanthanide An actinide A non-metal a. f. с. 3р d. 3d 111 SP 10:11 P 145 1135 Is 111113d SP P e. 3f f. 4s
Transcribed Image Text:1. The fact that most alpha particles passed directly through the foil in Rutherford's gold foil experiment led to the discovery that: a. the atom contains a large nucleus that takes up a majority of its space b. the atom is mostly empty space C. d. e. 2. An electron has the quantum numbers n= 3,1 2, m = 1,m, = +. In which orbital is this electron Hund's found? the atom contains electrons, which don't interact with alpha particles electrons orbit the nucleus in fixed energy level B & C a. 2p b. 3s 3. The orbital diagram to the right represents an electron configuration for: A transition metal An alkali metal An alkaline earth metal A lanthanide An actinide A non-metal a. f. с. 3р d. 3d 111 SP 10:11 P 145 1135 Is 111113d SP P e. 3f f. 4s
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