Inorganic Chemistry: Exam 1 Questions And Answers Study Guide PDF

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Dr. Jennifer Bubb...

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Exam 1 Study Guide 1. The name of the element with symbol “S” is a. sodium

b. sulfur c. silver d. selenium

e. none of these 2. Identify the SI units for each of the following: A. Volume = m3 B. Mass = kg C. Length = m D. Temperature = K 3. How many significant digits are in the following numbers? 1. 0.002650m A. 4

B. 5

C. 7D. 6

B. 5

C. 1D. 7

C. 3

C. 5D. 6

2. 43.026 g A. 4 3. 1044000 L A. 4

4. Perform the following calculation of measured numbers. Give the answer in (cm) the correct number of significant figures. (significant figures for x/÷)

A) 8.52

B) 8.5 C) 8.520

D) 9

5. Add the following measured numbers: (fewest decimal places +/-) 82.409 mg + 22.0

mg

A.104mg B. 104.4mg C. 104.41mg D. 104.409mg 6. Identify the larger unit in each of the following: 1. mm or cm

A. mm

B. cm

2. kilogram or centigram A. kg

B. cg

3. mL or μL

A. mL

B. μL

4. kL or mcL

A. kL

B. mcL

7. A rattlesnake is 2.44 m long. How many centimeters long is the snake? 1m = 100cm A. 0.0244 B. 244 C. 24.4 D. 2440 8. How many minutes are in 1.4 days? A. 33.6 B. 1440 C. 2016 D. 3600

9. If your pace on a treadmill is 65 meters per minute, how many minutes will it take for you to walk a distance of 7.5 kilometers?

A. 0.115 B. 115 C. 115.38 D. 120 10. Density= mass of substance volume of substance

Specific gravity= density of substance density of H2O

An unknown liquid has a density of 1.32 g/mL. What is the volume (mL) of a 14.7-g sample of the liquid? A. 11 B. 11.1 C. 19.4 D. 19 11. Identify each as a pure substance or a mixture: A. pasta and tomato sauce= heterogeneous mixture B. aluminum foil= pure substance C. helium= pure substance D. air= homogenous mixture 12. Identify each as a homogeneous or heterogeneous mixture: A. hot fudge sundae= heterogeneous mixture B. shampoo= homogeneous mixture C. dextrose solution= homogeneous mixture

D. peach pie= heterogeneous mixture 13. Identify each description as particles of a A) solid

B) liquid

1. definite volume, but takes the shape of the container= Liquid 2. particles are moving rapidly= Gas 3. particles fill the entire volume of a container= Gas 4. particles have a fixed arrangement= Solid 5. particles are close together, but moving randomly= Liquid 14. Identify the state of matter for each: A. vitamin tablets= Solid B. eye drops= Liquid C. vegetable oil= Liquid D. gold foil= Solid E. air in a tire= Gas 15. Classify each as a: A) change of state B) change of shape A. chopping a log into kindling= change of shape B. water boiling in a pot= change of state C. ice cream melting= change of state D. ice forming in a freezer= change of state E. cutting dough into strips= change of shape 16. Classify each change as: A. Physical 1. ice melting on the street= physical 3. toasting a marshmallow= chemical 4. cutting a salmon steak= physical

B. chemical

C) gas

5. iron rusting in an old car= chemical 17. Boiling point of water= 212°F or 373 K, Freezing point of water= 32°F or 0°C or 273 K 1. What is the temperature at which water freezes? A) 0 °F

B) 0 °C

C) 0 K

2. What is the temperature at which water boils? A) 100 °F

B) 32 °F

C) 373 K

3. How many Celsius units are between the boiling and freezing points of water? A) 100

B) 180

18. TF = 1.8TC + 32

C) 273 or

TC = TF – 32 or TK = TC + 273 1.8 On a cold winter day, the temperature is –15 °F. What is that temperature in degrees Celsius? A. −85 °C B. −47 °C C. −42 °C D. −26 °C 19. What is normal body temperature of 37 °C in kelvins? A. 236 K B. 310 K C. 342 K D. 98.0 K 20. 4.184 joules (J) = 1 calorie (cal) or 1 kJ = 1000 J or

1 kilocalorie (kcal) = 1000 cal

How many cal are obtained from a pat of butter if it provides 150 J of energy when metabolized? A. 0.36 cal B. 36 cal C. 630 cal D. 42 cal 21. A cup of whole milk contains 13 g of carbohydrate, 9.0 g of fat, and 9.0 g of protein. How many kilocalories does a cup of milk contain? (Round final answer to the tens place.) A. 50 kcal B. 80 kcal C. 170 kcal D. 270 kcal 22. Identify the element described by each of the following: 1. Group 7A, Period 4 A. Br B. Cl C. Mn 2. Group 2A, Period 3 A. beryllium

B. boron

C. magnesium

3. Group 5A, Period 2 A. phosphorus B. arsenic

C. nitrogen

23. Identify each of the following elements as a metal, nonmetal, or metalloid. A. sodium= Metal

B. chlorine= Nonmetal C. silicon= Metalloid D. iron= Metal E. carbon= Nonmetal 24. Select all of the elements that match each description. A. Metals in Group 4A B. Nonmetals in Group 5A

Sn, Pb, C, Si, Ge As, Sb, Bi, N, P

C. Metalloids in Group 4A C, Si, Ge, Sn, Pb 25. Which of the following subatomic particles fits each of the descriptions below? proton, neutron, electron A. found outside the nucleus= Electron B. has a positive charge= Proton C. has mass but no charge= Neutron 26. State the number of protons in a nitrogen atom. A) 5 protons

B) 7 protons

C) 14 protons

State the number of protons in a barium atom. A) 137 protons

B) 81 protons

C) 56 protons

27. An atom of lead (Pb) has a mass number of 207. A. How many protons are in the nucleus? 82 B. How many neutrons are in the nucleus? 207-82= 125 C. How many electrons are in the atom? 82 28. Write the atomic symbols for atoms with the following subatomic particles: A. 8 protons

8 neutrons

8 electrons = O

B. 17 protons 20 neutrons 17 electrons = Cl C. 47 protons 60 neutrons 47 electrons = Ag 29. 1. Which of the pairs are isotopes of the same element? = B 2. In which of the pairs do both atoms have eight neutrons? = C A.

B.

C.

30. Lithium consists of two naturally occurring isotopes, 6Li and 7Li. Use the periodic table to predict which isotope is the more prevalent one. Periodic table atomic mass of lithium is 6.941 amu.

A= 6Li B= 7Li

31. Gallium is an element found in lasers used in compact disc players. In a sample of gallium, there is 60.10% of 69Ga (atomic mass 68.926) atoms, 39.90% of 71Ga (atomic mass 70.925) atoms. What is the atomic mass of gallium? 69.72 amu 32. Electrons can move to higher energy levels when they: A) Absorb energy B) Emit energy 33. Write the electron arrangement for the following Si? A) 2, 6 B) 2, 4 C) 2, 8, 4 D) 2, 5 34. Number of valence electrons in aluminum is: A) 1

B) 2

C) 3

35. Given the following elements, answer the questions: A. Cl B. N

C. C

Which is the largest atom? C Which has the highest ionization energy? A Which belongs to Group 5A? B 36. Write the formula and symbol of an ion with 16 protons and 18 electrons. A = O2−

B = S2−

C = Sr2+

D = N3−

37. Consider the element calcium. A. Metal or a nonmetal? Metal B. Number of valence electrons? 2 C. Number of electrons that must be lost or gained to acquire an octet. Lose 2 D. Write the symbol including its ionic charge. Ca2+ 38. Select the correct formula for each of the following ionic compounds: 1. Na+ and O2− A) NaO

B) Na2O

C) NaO2

2. Al3+ and Cl− A) AlCl3

B) AlCl

C) Al3Cl

3. Mg2+ and N3− A) MgN

B) Mg2N3

C) Mg3N2

39. Write the names of the following compounds. A. CaO Calcium oxide B. Al2O3 Aluminum oxide C. MgCl2 Magnesium chloride 40. Name the following ionic compounds containing metals that form two kinds of positive ions: A. Fe2O3 Iron(III) oxide B. SnCl2 Tin(II) chloride 41. Write chemical formulas for the following compounds:

A. Nickel(II) sulfide= NiS B. Zinc chloride= ZnCl2 C. Iron(III) oxide= Fe2O3 42. Select the correct formula for each. 1. aluminum nitrate A) AlNO3

B) Al(NO)3

2. copper(II) nitrate A) CuNO3

B) Cu(NO3)2 C) Cu2(NO3)

3. iron(III) hydroxide A) FeOH

B) Fe3OH

4. tin(IV) hydroxide A) Sn(OH)4 B) Sn(OH)2

C) Al(NO3)3

C) Fe(OH)3 C) Sn4(OH)

43. Name each of the following compounds containing polyatomic ions. A. MgSO3 Magnesium Sulfite B. MgSO4 Magnesium sulfate C. Ca(ClO3)2 Calcium(II) chlorate 44. Select the correct name for each compound. 1.SiCl4

2. P2O5

3.Cl2O7

A)

silicon chloride

B)

tetrasilicon chloride

C)

silicon tetrachloride

A)

phosphorus oxide

B)

phosphorus pentoxide

C)

diphosphorus pentoxide

A)

dichlorine heptoxide

B)

dichlorine oxide

C)

chlorine heptoxide

45. Write the correct formula for each of the following:

A. phosphorus pentachloride= PCl5 B. dinitrogen trioxide= N2O3 C. sulfur hexafluoride= SF6 46. Use the electronegativity difference to identify the type of bond [nonpolar covalent (NP), polar covalent (P), or ionic (I)] between the following: A. K-N Ionic B. N-O Covalent polar C. Cl-Cl Covalent nonpolar D. H-Cl Covalent polar 47. Identify each of the following molecules as polar or nonpolar: A. PBr3= Polar B. HBr= Polar C. CF4= Nonpolar 48. Identify the main type of attractive forces that are present in liquids of the following compounds: ionic bonds, dipole–dipole, hydrogen bonds, or dispersion forces. A. NCl3 = Dipole-dipole B. H2O = Hydrogen bond C. Br—Br = Dispersion forces D. KCl = Ionic E. NH3 = Hydrogen bond 49. The number of atoms in 2.0 mole of Al atoms is: A. 2.0 Al atoms B. 3.0 x 1023 Al atoms

C. 1.2 x 1024 Al atoms 50. The number of moles of S in 1.8 x 1024 atoms of S is: A. 1.0 mole of S atoms B. 3.0 moles of S atoms C. 1.1 x 1048 moles of S atoms 51. How many atoms of O are in 0.150 mole of aspirin, C9H8O4? 3.61 atoms O 52. Calculate the molar mass of C2H6O. 46.07 g/mol 53. A sample of water has a mass of 59.8 grams. How many moles of water are in the sample? 3.32 mol H2O 54. Balance and list the coefficients from reactants to products. A. __Fe2O3(s) + __C(s) 1) 2, 3, 2, 3

__Fe(s) + __CO2(g)

2) 2, 3, 4, 3

B. __Al(s) + __FeO(s) 1) 2, 3, 3, 1

__Fe(s) + __Al2O3(s)

2) 2, 1, 1, 1

C. __Al(s) + __H2SO4(aq) 1) 3, 2, 1, 2

3) 1, 1, 2, 3

2) 2, 3, 1, 3

3) 3, 3, 3, 1 __Al2(SO4)3(aq) + __H2(g) 3) 2, 3, 2, 3

55. Classify each of the following reactions as combination, decomposition, single replacement, double replacement, or combustion. A. 2Al(s) + 3H2SO4(aq)



Al2(SO4)3(s) + 3H2(g) = Single replacement

B. Na2SO4(aq) + 2AgNO3(aq)  

C. N2(g) + O2(g)

D. C2H4(g) + 3O2(g) 

Ag2SO4(s) + 2NaNO3(aq) = Double replacement

2NO(g) = Combination 2CO2(g) + 2H2O(g) = Combustion

56. Identify each of the following as oxidation or reduction: 

Sn4+(aq) + 4e− = Oxidation

1.

Sn(s)

2.

Fe3+(aq) + 1e−

3.

Cl2(g) + 2e− 



Fe2+(aq) = Reduction 2Cl− (aq) = Reduction

57. How many moles of Fe are needed for the reaction of 12.0 moles of O2? 4Fe(s) + 3O2(g)

2Fe2O3(s)

A. 3.00 moles of Fe B. 9.00 moles of Fe C. 16.0 moles of Fe 58. How many grams of O2 are needed to produce 45.8 grams of Fe2O3 in the following reaction? 4Fe(s) + 3O2(g) A. 38.4 g of O2 B. 13.8 g of O2 C. 1.38 g of O2

2Fe2O3(s)

Important Formulas 

Density= mass of substance volume of substance



TF = 1.8TC + 32

Specific gravity= density of substance density of H2O

or



TC = TF – 32 1.8 Atomic number = number of protons

or TK = TC + 273



Mass number = number of protons + number of neutrons



Atomic mass = percent abundance x atomic mass of isotope then sum the total mass of each isotope



Energy Levels = n=1 2n2 so 2(12) = 2en=2  2(22) = 8en=3  2(32) = 18e-



Valence electrons = group number



Atomic size = increases top to bottom, decreases left to right “F is the smallest”



Ionization energy = decreases top to bottom, increases left to right “F has the highest”



Metallic character = increases top to bottom, decreases left to right “F has the least”



Metals form positive ions = 1A lose 1 e- 1+ 2A lose 2 e- 2+ 3A (B + Al) lose 3 e- 3+





Nonmetals form negative ions = 5A  gains 3 e-  3And suffix becomes “ide” 6A gains 2 e- 27A gains 1 e- 1Diatomic molecules = H7



Electronegativity = decreases top to bottom, increases left to right (nonmetals/high & metals/low)



1 mole of an element = 6.02 x 1023 atoms of that element



covalent compounds  molecules, ionic compounds  formula unit (or molecule)



Molar mass = g / mol



Oxidation is loss of e- , Reduction is gain of e-...