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Chemistry 1 Pre-AP Semester Review
1.
Consider the chemical reaction in which carbon reacts with oxygen to produce carbon dioxide.
What mass of carbon dioxide would be produces if 24 grams of carbon reacted completely with 64
grams of oxygen
a. 40 g
b. 48 g
c.130 g
d. 88 g
e. 64 g
2.
If the number 53.4 is multiplied by the number 2.11; how many digits should the answer
contain?
a. 1
b. 2
c. 3
d. 4
Round each of the following numbers to 3 significant digits.
a. 1995.6 m
b. 0.0045921 kg
c. 326.001 cm
d. 3010.0 m
If the atomic mass of a neutral atom of chlorine is 35 amu, how many neutrons does it
have?
a. 17
b. 18
c. 35
d. 52
What is the energy of a photon of red light with a wavelength of 6.45 x 10-5 cm?
a. 3.08 x 10-19 J
b. 3.08 x 10-21 J
c. 4.28 x 10-38 J
d. 7.02 x 1047 J
Make the conversions indicated:
a) 6.00 x 104 μm = ________ m
b) 2.2 nm = ____________Tm
3.
4.
5.
6.
c)27.6 ml = ___________L
e) 531 mg = ___________kg
d) 7.53 L = ___________cm3
f) 6.7 Mg = ____________cg
7. What is the approximate volume of a sample of element Q that has a
mass of 10g?
a. 6 cm3
b. 10 cm3
c. 15 cm3
d. none of the above
8. A student tests an unknown substance. The properties she tested and her
results are shown in the table. Given this information, which of the
following is the most reasonable conclusion for the student to reach?
Ductility
Compressibility
Melting Point
Density
Average kinetic energy of particles
a. the substance is a solid
c. the substance is a liquid
Ductile
Noncompressible
High
13.6 g/cm3
Low
b. the substance is a plasma
d. the substance is a gas
Chemistry 1 Pre-AP Semester Review
9. Mr. Jones goes into Denny’s and orders tea with his lunch. He likes his
tea really sweet and will need to add sugar. Which combination of tea and
sugar should he use to produce the sweetest solution of tea?
a. granulated sugar and hot tea
b. sugar cube and hot tea
c. granulated sugar and cold tea
d. sugar cube and cold tea
10. Which of the following would compress a gas?
a. heating
b. cooling
c. melting
d. increasing the size of the container
11. A student is working with four beakers that each contains a clear liquid.
Which set of procedures would be best to use to determine whether one of
the beakers contains only distilled water?
a. Observe odor, determine temperature, observe color, determine boiling
point
b. Observe odor, determine pH, determine density, determine boiling point
c. Observe volume, determine mass, observe color, determine pH
d. Determine mass, observe volume, determine temperature, observe
color
12. An open container of water is brought to a boil and heated until all of the water is
converted to water vapor. Which of the following describes the changes in the
water molecules?
a. The molecules speed up and move farther apart
b. The molecules speed up and move closer together
c. The molecules slow down and move farther apart
d. The molecules slow down and move closer together
13. Which of the following is not part of the kinetic theory?
a. particles are always moving
b. particles are smaller at lower pressure
c. particles move faster at higher temperatures
d. all matter is made up of tiny, invisible particles
14.
Chemistry 1 Pre-AP Semester Review
A piece of metal is heated in a Bunsen burner flame and then immersed in a beaker of cool
water. Which statement best describes the effect of the temperature changes on the kinetic
energy of the particles?
a. Kinetic energy of metal atoms decreases in the flame
b. Kinetic energy of water molecules increases when the heated metal is immersed
c. Kinetic energy of water molecules decreases when the heated metal is immersed
d. Kinetic energy of metal atoms increases when immersed in the cooler water
15. According to Billy Mays, Oxyclean is better at removing organic compound stains from
clothes than other detergents. Most organic compounds are nonpolar. What can you
surmise about Oxyclean?
a. it is a polar molecule
b. it is a nonpolar molecule
c. it is a neutral molecule
d. not enough information to tell
16. The diagram above represents radiation passing through and electric field as in
experiments performed by Thomson, Rutherford and Millikan. The scientists reasoned
that the arrow labeled A most likely represents:
a. an electron
b. gamma radiation
c. a proton
d. a neutron
Element
Reaction with vinegar
Bonds easily with halogens
A
Yes
Yes
B
yes
No
C
No
No
D
Yes
yes
17. If Mendeleev found the above data to be true, which 2 elements would he place in the
same family/group?
a. A and B
b. B and C
c. A and D
d. B and C
18. The data table below provides some properties of unknown elements A,B,C and D.
Evaluate and determine which element is most likely a nonmetal.
a. A
b. B
c. C
d. D
Chemistry 1 Pre-AP Semester Review
19. From the list below, choose the discovery and the scientist(s) primarily
responsible for each model of the atom.
Models
Plum pudding
Planetary
Quantum Mechanical
Scientists
Discoveries
Thomson
Millikan
Goldstein
Rutherford
Bohr
Schrodinger
Heisenberg
Atom
Electron
Proton
Neutron
Nucleus
Wave equation
Law of octaves
20. Ernest Rutherford performed a famous experiment in which he used a radioactive
alpha particle source and aimed the particles at a thin sheet of gold foil. . By
studying photographic plates placed around the foil, he found that most particles
passed straight through; some were reflected straight back to the source. The
discovery led Rutherford to make several important conclusions. Using the
experimental set-up shown above, what conclusions about atoms were made by
Rutherford?
a. each atom contains electrons
b. each atom contains protons
c. the nucleus of an atom can be split
d. atoms are mostly empty space
21. Identify the number of subatomic particles in each of the following:
14. I-131
15. O216. Rb1+
17. Fe3+
22. What is the frequency of a photon of light given off by an electron that glows
orange with a wavelength of 575 nm?
How much energy (in joules) would it take for that electron to regain the energy
level it just descended from?
Chemistry 1 Pre-AP Semester Review
23. What would be the quantum address for an electron found in the fourth energy
level, the p sublevel, the center orbital with a clockwise spin?
24. What is the difference between an electron in its excited state and that same
electron in its ground state?
25. Why do the elements sodium and lithium have similar chemical properties?
a. same number of protons
b. similar atomic masses
c. same ratio of protons to electrons
d. same number of valence electrons
26.
Consider the hypothetical element Cp. If Cp generally forms an ion with a charge of -3, what
would you deduce to be the Lewis electron dot formula for the neutral atom?
a.
.
. Cp :
.
b.
..
: Cp :
..
c.
..
Cp
.
d.
:
. Cp :
.
27. IF 75.4% of naturally occurring chlorine atoms have an atomic mass of 35.012 and the
rest have an atomic mass of 37.134, what is the atomic mass of chlorine?
28. If the wavelength of a band of light is relatively long, what can we predict about
the frequency of that wave?
a. it will be relatively low
b. it will be relatively high
c. we cannot predict
d, it will be sometimes high and sometimes low
29. What would be the wavelength, in nanometers, of light that has a frequency of 6.42 x
1014?
30. A neutral atom of fluorine has the same number of electrons as which of the following?
a. B3b. N1+
c. Ne1d. Na1e. Mg3+
31. What determines how much energy is given off as an excited electron returns to
its ground state?
32. A (an) __________ is an atom that has a different number of electrons than usual.
33. A(an) _______________ is an atom that has a different number of neutrons than usual.
34. A(an) _________________ is the amount of visible light given off as an electron moves
from its excited state to its ground state
35. A(an) _______________ is the amount of energy it takes to move an electron from one
energy level to another
36. When the Cu-67 atom oxidizes to form a 2+ ion, it contains ______ electrons, ______
protons, and _____ neutrons.
Chemistry 1 Pre-AP Semester Review
37. IF 57.25% of naturally occurring antimony atoms have an atomic mass of 210.9038 and
the rest have an atomic mass of 212.9041, what is the average atomic mass of antimony?
38. For the ion Br1-, show the orbital distribution diagram, write the electron configuration,
draw the Lewis electron dot diagram and identify the distinguishing electron by its
quantum numbers.
39. If a photon of light given off by an atom has a wavelength of 655nm, what would be the
energy of that lightwave?
40. When using the spectrometer we noticed that depending upon which elemental gas is
used to produce the light, different lines of the spectrum will appear. If the predominant
band is red, what could you hypothesize about the waves that created these bands with
regard to energy and wavelength?
41. Within a family of elements, the electronegativity __________ as the atomic number
increases.
42. Within a period, the atomic radius __________ as the atomic number increases.
43. As a nonmetal becomes an ion, its radius _________
44. The ______________ are the family that contain the most reactive metals.
45. Examine the following electron configuration for element X and use it to answer the
questions below 1s22s22p63s23p64s23d104p65s24d2
a. In which period is element X?
b. What is the atomic number of element X?
c. How many electrons are in the outer energy level of element X?
46. For the following groups of elements, select the one that has the property noted:
a. the largest atom of H, Ar, Ag, Ba, Te, Au
b. the lowest first ionization energy of B, Sr, Al, Br, Mg, Pb
c. the greatest electron affinity of Na, I, Ba, Se, Cl, P
d. the highest electronegativity of As, Ca, I, P, Ga, Se, Sn
e. the largest number of unpaired electrons of F, N, S2-, Mg2+, Sc3+, Ti3+
47. How would you characterize arsenic with regards to electronegativity, ionization
energy and atomic radius?
How would you characterize barium?
How would you characterize argon?
48. Tin is in group 4 and period 5. What is the electron configuration of its outermost energy
level?
49. Given two elements, how would you determine the type of bond that would form
between them?
Chemistry 1 Pre-AP Semester Review
50. Compare and contrast the properties of the compounds formed (including how the
bond forms between them) in ionic and molecular compounds.
51. Describe in detail, including examples of substances exhibiting each, the
attractive forces below.
a. metallic bonding
b. van der Waal forces
c. dipole interaction
d. dispersion forces
e. hydrogen bonding
52. Identify each of the following compounds as to type of bond: ionic, nonpolar covalent, or
polar covalent.
Draw the electron dot diagram/structure for each substance - identify the shape and
polarity of the molecules.
a. HI
b. RbCl
c. GeCl4
d. PH3
e. H2Se
f. BeCl2
g. SO2
h. Na2S
53. The basis of the gas laws revolves around the properties of volume, pressure and
temperature, and how these properties are affected by the kinetic molecular theory.
Describe the relationship between each pair of properties.
a. temperature and pressure
b. temperature and volume
c. pressure and volume
54. The physical state of a substance depends mostly on its ________ at room
temperature and standard pressure.
a.container
b. density
c . molecular mass
d. bonding structure
55. Even at low temperature, a ______ particle travels in a completely random
manner.
a. liquid
b. gas
c. solid
d. plasma
56. The average kinetic energy of water molecules is greatest in which of the
following?
a. Steam at 100C
b. water at 90C
c. water at 373K
d. ice at 0C
57. A nonpolar solvent will most likely dissolve a(n) _________ solute?
a.nonpolar
b. polar
c. ionic
d. metallic
Chemistry 1 Pre-AP Semester Review
58. Which of the following could affect both the rate of solution and the solubility of
a solid in a liquid?
a. stirring the mixture
b. increasing the pressure
c. increasing the surface area
d. increasing the temperature
59. As pressure increases, what happens to the solubility of gases in liquids?
a. decreases
b. increases
c. decreases and then increases
d. remains the same
60.
Which of the following is not an electrolyte?
a. Cl2(aq)
b. HCl(aq)
c. NaCl(l)
d. (NH4)2SO4(aq)
61. Consider three identical flasks filled with different gases.
Flask A: CO at 101.3 kPa and 0ºC
Flask B: N2 at 30.7 kPa and 0ºC
Flask C: H2 at 13.3 kPa and 0ºC
a. In which flask will the molecules have the greatest average kinetic energy
b. In which flask will the molecules have the greatest number of collisions per
second with the walls of the container?
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