8.1 Multiple-Choice and Bimodal Questions 1) There are __________ paired and __________ unpaired electrons in the Lewis symbol for a phosphorus atom. A) 4, 2 B) 2, 4 C) 2, 3 D) 4, 3 E) 0, 3 Answer: C Diff: 1 Page Ref: Sec. 8.1 2) In the Lewis symbol for a fluorine atom, there are __________ paired and __________ unpaired electrons. A) 4, 2 B) 4,1 C) 2, 5 D) 6, 1 E) 0, 5 Answer: D Diff: 1 Page Ref: Sec. 8.1 3) Based on the octet rule, magnesium most likely forms a __________ ion.
k. What is the hydroxide concentration of a substance with a pOH of 8.5? 5. Write the dissociation equation for each of the following: l. sodium sulfate m. magnesium hydroxide n. calcium bromide. 6. Draw the Lewis structure for CH3Cl.
6. Copper has two stable isotopes,[pic]and [pic], with masses of 62.939598 amu and 64.927793 amu, respectively. Calculate the percent abundances of these isotopes of copper. 7. Chromium has four naturally occurring isotopes: chromium – 50 (4.35% at 49.946 amu) chromium – 52 (83.79% at 51.941 amu) chromium – 53 (9.50% at 52.941 amu), and chromium – 54 (2.36% at 53.939 amu) Calculate the average atomic mass of
104 kJ/mol C. 52 kJ/mol D. -52 kJ/mol E. -104 kJ/mol 59. Give the number of lone pairs around the central atom and the molecular geometry of SCl2. A. 0 lone pairs, linear B. 1 lone pair, bent C. 2 lone pairs, bent D. 3 lone pairs, bent E. 3 lone pairs, linear 60.
What is the quantity 987 milligrams expressed in grams? Use the table above to help you. a.|0.000 987 g|c.|9.87 g| b.|0.987 g|d.|98,700 g| 11. The quantity 44 liters expressed in cubic meters is ____. a.|0.000 044 m|c.|0.44 m| b.|440 000 m|d.|0.044 m| 12.
Mg = 24 g/mole Percent of an element = Mass of the element X 100 C = 12 g/mol Total formula mass O = 16 g/mol 3. How many grams are there in 0.5 moles of each of the compounds? a) H2S b) Mg c) C12H22O11 d) F2 4. How many particles
STA: SC.912.N.3.5 | SC.912.P.8.5 BLM: comprehension 56. ANS: A PTS: 1 DIF: L2 REF: p. 272 | p. 280 OBJ: 9.2.1 Apply the rules for naming and writing formulas for binary ionic compounds. | 9.3.1 Apply the rules for naming and writing formulas for binary molecular compounds. STA: SC.912.P.8.7 | SC.912.N.1.1 | SC.912.N.1.6 | SC.912.P.8.7 BLM: application 57. ANS: B PTS: 1 DIF: L2 REF: p. 276 | p. 277 | p. 278 OBJ: 9.2.2 Apply the rules for naming and writing formulas for compounds with polyatomic ions.
8. Calculate the relative mass of each isotope by multiplying its relative abundance by its average mass. 9. Calculate the weighted average mass (atomic mass) of all candium particles by adding the relative masses. A(blue) B(orange) C(red) Total Total Mass(g) 28.05g 8.58g 7.3g 43.93g Number 32 11 8 51 Average Mass(g) 0.876g 0.78g 0.913g 0.861g Relative Abundance 0.6275 0.2157 0.1569 1.000 % Percent Abundance 62.75% 21.57% 15.69% 100% Relative Mass(g) 0.5497g 0.1682g 0.143g 0.8608g IV.
CH4 4+4(1)=8 H H C H H 1. What is the central atom? (1 point for each molecule) The central atom is C. 2. How many atoms are bonded to the central atom? (1 point for each molecule) There are four atoms bonded to the central atom.
N05/4/PHYSI/SPM/ENG/TZ0/XX+ The mass of an atom of the isotope strontium-92 (92Sr) is of the order of A. B. C. D. 10–23 kg. 10–25 kg. 10–27 kg. 10–29 kg.