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Exam I Review

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An element cannot be broken down into two or more pure substances ... Iridium. Cesium. Manganese. 14. How many metals are there in group 13? 0. 1. 2. 3. 4 ... – PowerPoint PPT presentation

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Title: Exam I Review


1
Exam I Review
  • Chemistry 1211
  • Dr. Clower

2
  • 1. All of the following are true except
  • An element cannot be broken down into two or more
    pure substances
  • A compound is a substance that contains two or
    more elements
  • A pure compound always contains the same elements
    in the same mass percentages
  • Another name of a heterogeneous mixture is a
    solution

3
  • 2. All of the following statements are true
    except
  • Potassium is represented by the symbol K
  • Zinc is represented by the symbol Zn
  • Argon is represented by the symbol Ar
  • Iron is represented by the symbol Fe
  • Nitrogen is represented by the symbol Ni

4
  • 3. All of the following relationships are false
    except
  • 1.5 cm3 1.5 mL
  • 3.00 m3 lt 3.00 L
  • 5.2 m3 5.2 x 102 cm3
  • 0.0455 L gt 455 mL
  • 22 L 22 m3

5
  • 4. If the outdoor temperature is 17.0ºC, what is
    the temperature in Fahrenheit?
  • -1.40ºF
  • 30.6ºF
  • 41.4ºF
  • 62.6ºF
  • 74.6ºF

6
  • 5. How many significant figures are in the
    following mass 0.00047800 kg?
  • 3
  • 5
  • 6
  • 8
  • 9

7
  • 6. What is the correct answer to the expression
    below?
  • 8 cm
  • 7.8 cm
  • 7.83 cm
  • 7.826 cm
  • 7.8257 cm

8
  • 7. How many miles are covered in a 15 km race?
  • 7.1 mile
  • 9.3 mile
  • 11 mile
  • 15 mile
  • 26 mile

9
  • 8. Which of the following describes a chemical
    change?
  • Oxygen reacts with aluminum, forming a protective
    coating
  • The density of mercury metal is 13.534 g/cm3
  • Ethyl alcohol evaporates from a beaker
  • The melting point of sodium chloride is 801ºC
  • Both answers A and D are correct

10
  • 9. A solid with a mass of 19.3 g is added to a
    graduated cylinder filled with water to the 25.0
    mL mark. After the solid sinks to the bottom, the
    water level is at 35.8 mL. What is the density of
    the solid?
  • 0.539 g/mL
  • 0.560 g/mL
  • 1.79 g/mL
  • 2.19 g/mL
  • 8.50 g/mL

11
  • 10. All of the following statements are true
    except
  • A proton carries a 1 charge and an electron
    carries a -1 charge
  • The nucleus of an atom has a negative charge
  • A neutron is an uncharged particle with a mass
    slightly greater than a proton
  • More than 99.9 of an atoms mass is concentrated
    in the nucleus

12
  • 11. All atoms of the same element have the same
    number of __________.
  • Neutrons
  • Protons
  • Protons and neutrons
  • Electrons and neutrons
  • Protons, neutrons, and electrons

13
  • 12. A radioactive isotope of fluorine, 20F, has
  • 9 protons, 10 neutrons, and 1 electron
  • 9 protons, 10 neutrons, and 9 electron
  • 9 protons, 11 neutrons, and 9 electron
  • 10 protons, 9 neutrons, and 1 electron
  • 10 protons, 10 neutrons, and 10 electron

14
  • 13. What is the identity of the following
    element?
  • Zinc
  • Silver
  • Iridium
  • Cesium
  • Manganese

15
  • 14. How many metals are there in group 13?
  • 0
  • 1
  • 2
  • 3
  • 4

16
  • 15. Which group of three elements contains an
    alkaline earth metal, a halogen, and an inner
    transition metal?
  • Be, S, U
  • Ba, As, Ce
  • U, Cl, Rb
  • Mg, Br, Pu
  • K, Ga, Se

17
  • 16. A strontium ion has _______ electrons.
  • 36
  • 37
  • 38
  • 39
  • 40

18
  • 17. What is the charge on a sulfide ion?
  • -2
  • -1
  • 0
  • 1
  • 2

19
  • 18. Identify the ions and their charges in
    Na2SO4.
  • Na, SO4-
  • Na, SO42-
  • Na, SO4-
  • Na2, SO4-
  • Na2, SO42-

20
  • 19. What is the correct name for K3PO4?
  • Tripotassium phosphate
  • Potassium (I) monophosphorus tetraoxide
  • Potassium (I) phosphate
  • Potassium phosphate
  • Potassium pohsphide

21
  • 20. What is the correct name for N2O3?
  • Nitrogen oxide
  • Nitrogen (II) oxide
  • Nitrogen (III) oxide
  • Trioxygen dinitride
  • Dinitrogen trioxide

22
  • 21. What is the formula for chlorous acid?
  • HCl
  • HClO
  • HClO2
  • HClO3
  • HClO4

23
  • 22. An atomic mass unit (amu) is defined as
  • 1.602 10-19 C
  • The mass of 1 mole of hydrogen-1 atoms
  • The mass of 1 hydrogen-1 atom
  • The mass of 1 carbon-12 atom
  • 1/12 the mass of 1 carbon-12 atom.

24
  • 23. An element has three naturally occurring
    isotopes with the following abundances and
    masses. Determine the atomic mass of the element.
  • Abundance mass(amu)
  • 78.99 23.985042
  • 10.00 24.985837
  • 11.01 25.982593
  • 24.31 amu
  • 24.98 amu
  • 74.95 amu
  • 2431 amu
  • None of the above

25
  • 24. Which one of the following is the most
    effective method of determining isotopic ratios
    of elements?
  • Distillation
  • Filtration
  • Chromatography
  • Absorption spectroscopy
  • Mass spectrometry

26
  • 25. Which of the following samples contains the
    largest number of atoms?
  • 2.0 moles of H3PO4
  • 3.0 moles of H2SO3
  • 4.0 moles of HNO3
  • 6.0 moles of HClO
  • 8.0 moles of HBr

27
  • 26. What mass of oxygen is present in 10.0 grams
    of carbon dioxide?
  • 0.227 g
  • 4.64 g
  • 4.40 g
  • 7.27 g
  • 8.80 g

28
  • 27. Which is a correct method for determining the
    mass in grams of 0.190 mol silver?
  • None of the above

29
  • 28. Which is a correct method for determining the
    total number of atoms in 123 grams of sulfur
    trioxide?

30
  • 29. What is the percent composition of silicon
    nitride (Si3N4)?
  • 30.21 Si and 69.79 N
  • 42.92 Si and 57.08 N
  • 54.03 Si and 45.97 N
  • 60.06 Si and 39.94 N
  • 69.40 Si and 30.60 N

31
  • 30. A mass of 8.15 g C2H4(g) reacts with excess
    oxygen. If 16.2 g CO2(g) is collected, what is
    the percent yield of the reaction?
  • C2H4(g) 3O2(g) ? 2CO2(g) 2H2O(g)
  • 25.6
  • 31.7
  • 41.0
  • 57.1
  • 63.3

32
  • 31. An oxide of nitrogen contains 63.1 oxygen
    and has a molar mass of 76.0 g/mol. What is the
    molecular formula for this compound?
  • N2O
  • NO
  • NO2
  • N2O3
  • N2O5

33
  • 32. Hydrazine, a fuel used to power rocket
    engines, is a product of the reaction between
    ammonia and bleach. Balance the equation for the
    reaction.
  • aNH3(aq) bOCl-(aq) ? cN2H4(l) dCl-(aq)
    eH2O(l)
  • a 2, b 1, c 1, d 1, e 1
  • a 2, b 2, c 1, d 2, e 2
  • a 2, b 1, c 2, d 1, e 2
  • a 4, b 3, c 1, d 3, e 1
  • a 4, b 3, c 2, d 3, e 2

34
  • 33. Aluminum reacts with oxygen to form aluminum
    oxide. Which of the reactions below is correct
    and properly balanced?
  • Al(s) O(g) ? AlO(s)
  • 2Al(s) O2(g) ? 2AlO(s)
  • 3Al(s) O2(g) ? Al3O2(s)
  • 4Al(s) O2(g) ? 2Al2O(s)
  • 4Al(s) 3O2(g) ? 2Al2O3(s)

35
  • 34. Which method is correct for determining the
    mass of carbon dioxide that can be made by the
    combustion of 3.219 grams of ethanol with excess
    oxygen?
  • C2H5OH(l) 3O2(g) ? 2CO2(g) 3H2O(l)
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