Chemistry Semester 1 Final Exam review



Chemistry Semester 1 Final Exam review Name____________________________ per_____

1. What is a definition of Chemistry?

2. Matter includes all of the following EXCEPT:

a. air b. light c. smoke d. water vapor

3. What are two factors that distinguish matter?

4. Define a physical change. ________________________________________________________ Define a chemical change. ________________________________________________________ Label which are physical changes and chemical changes:

a. peach spoils_____ b. copper bowl tarnishes______ c. bracelet turns wrist green_____ d. glue gun melts a glue stick____

5. The particles in a solid are

a. packed closely together b. constantly in motion c. very far apart d. able to slide past one another

6. Physical means may be used to separate __________________________ and they include ________________, ______________________, ______________________, ___________________

Of the following groups, 1, 2, 14, 15, 17, 18:

7. Group(s) __________ contains only metals

8. Group (s)__________is called a Noble gases

9. Group(s) __________has 7 electrons on the valence shell

10. Group(s) __________needs to gain 3 electrons to fill a stable octet

11. Group(s) __________has a 2+ oxidation state

12. Group(s) __________has an electron dot notation of [pic]X

13. Using the periodic table, an element similar to carbon would be_______

14. Based on their location on the periodic table, you could infer that _____________is very unreactive

15. The horizontal row on the periodic table is called a(n)______________________________

16. The vertical column of blocks on the periodic table is called a(n)____________

17. The elements on the zigzag line in the periodic table are ________________

18. Which is NOT a property of metal?

a. malleability b . unreactive c. ability to lose electrons d. ability to conduct heat

19. The validity of scientific concepts is evaluated by

a. collecting facts c. voting by scientists

b. providing explanations d. testing hypotheses

20. All but one of these units are SI base units. The exception is

a. kilogram b. second c. liter d. Kelvin

21. The symbol for the metric unit used to measure mass in the Chemistry lab is

a. m b. mm c. g d. L

22. The quantity that describes the concentration of matter is

a. weight b. density c. volume d. mass

23. Convert: a) 2.5 liters into mL_______________ b) 6.2 x 104 microliters to Liters_______________ c) 0.5 kg to g __________

24. A volume of 1 cc (cm3) is the same as _______________mL

25. To determine density, the quantities that must be measured are ___________ and _____________

26. The relationship between the mass m of a material , its volume V, and its density D is

a. V = mD b. Vm = D c. DV = m d. D + V = m

28. The density of aluminum is 2.70 g/cm3. The volume of a solid piece of Aluminum is 1.50 cm3. Find the mass

27. The density of pure diamond is 3.5 g/cm3. The mass of a diamond is 0.25 g. Find the volume

28. What statement about density is true?

a. two samples of a pure substance may have different densities if they are different sizes

b. the density of a sample depends on its location on Earth

c. a cylinder is always used to measure the volume

d. density is a physical property that remains constant for a pure substance

29. The number of grams equal to 0.5 kg is ___________

30. 30oC = ________________K

31. A measurement that closely agrees with accepted values is said to be ____________ (accurate or precise)

32. In Chemistry, the quantitative labs need to have a confidence level of _____________

33. The equation for percent error is _____________________________________________________________________

34. Calculate the percent error if you found the density of water to be 1.08 g/ml and the actual density of water is 1.0g/ml.

35. Calculate the average atomic mass of an element with two isotopes. One isotope has a mass of 45 amu and an abundance of 44%. The second isotope has a mass of 44 amu and a relative abundance 56%.

36. The variable that you change in the lab is the _______________variable. The variable that responds to the change is called the _________________variable. All other things do not change and are called _________

37. At first Dalton thought the atom was _________________, then Ruther ford discovered the ___________ of the atom, then the subatomic particles _______________, ___________, and __________ were discovered

38. The positively charged particle is the _________________ found in the ______________ of the atom

39. The subatomic particle that has about the same mass as the proton, but with no electrical charge, is called a __________________ and is found in the _________ of the atom

40. The _______________is negatively charged and is found in the _____________ of the atom

41. _____________is the person credited with placing electrons on levels and ____________ established the electron cloud theory.

42. The forces that hold the particles together in the nucleus are ________________ forces

43. Isotopes are atoms of the same element that ____________________________________

44. All isotopes of hydrogen contain ____________________

45. What is the atomic number for Nitrogen? _______________To what subatomic particle does this correspond?

46. Zinc –66 has ________protons and __________neutrons

47. The number of atoms in 1 mole of carbon is _______________________________

48. The mass of 1 mole of Chromium is ______________

49. The mass of 3.5 moles of silicon is ___________________

50. What is the electron configuration for sodium? Chlorine? Neon?

51. What is the dot notation for magnesium? Bromine? Argon?

52. How many electrons is each element trying to achieve in the valence level?

53. Who is given credit with developing the modern periodic table? _______________How was it arranged?_______________

54. Which family is entirely radioactive?

55. Which family will gain two electrons to complete their octet?

56. Where are the transition metals located? What is special about their electron configuration that gives them special properties?

57. As you move left to right across a period on the table the size (radius) __________________

58. As you move down a column(group) the ionization energy _______________________

59. The most active metal is ______ and the most active nonmetal is ___________

60. As atoms bond with each other, they

a. increase their potential energy, thus creating less-stable arrangements of matter

b. decrease their potential energy, thus creating less-stable arrangements of matter

c. increase their potential energy, thus creating more-stable arrangements of matter

d. decrease their potential energy, thus creating more-stable arrangements of matter

75. When atoms share electrons, a ______________ bond is formed

76. When ________ electrons are shared a triple covalent bond is formed

77. Covalent bonds may be equally shared called _____________ and unequally shared called ________

78. The most common example of an unequally shared covalent material is ________________

79. Define ionic bond and metallic bond.

80. What are characteristics of a covalent bond, an ionic bond and a metallic bond (list on another paper)

81. What is an exothermic reaction? _____________________What is an endothermic reaction?____________________

82. Changing a subscript in a correctly written chemical formula

a. changes the number of moles represented by the formula b. changes the charges on the other ions in the compound

c. changes the formula so that it no longer represents that compound d. has no effect on the formula

83. Technetium-99 has been used as a radiographic agent in bone scans (9943Tc is absorbed by bone). If 9943Tc has a half-life of 6.0 hours how much of a 100µg sample would remain in the patient’s body after 2.0 days?

84. Silicon-31 has a half-life of 2.5 hours. If we begin with a sample containing 1000mg of Si-31 how much will remain after 10 hours?

85. What are α, β, γ particles?

86. Rank α, β, γ radiation in order of increasing energy (from lowest to highest).

87. 3717Cl → 3718Ar + _____ 3315P → _____ + 3215P 23893Np + 0-1β → ________

88. _____ → 18776Os + 0-1β 23893Np → ________ + 0-1β

89. 136C → ____ + 42He 23692U → 9436Kr + ________ + 310n

General Chemistry Fall Final Exam Study Guide (Ch.1-6 and Ch.21)

Ch1: Matter and Change

Vocab: chemical, matter, atom, chemical change, physical change, reactant, product

Periodic Table: Groups/Families, Periods, Alkali Metals, Alkaline Earth Metals, Halogens, Noble Gases, Metals, Nonmetals, Transition Metals, Inner Transition Metals, Lanthanides, Actinides, Metalloids, Representative Elements

Mixtures: Homogenous/Solutions, Heterogeneous

Pure Substances: atoms, compounds

Conservation of Mass, Law of Definite Proportions

Ch2: Measurements and Calculations

Vocab: quantitative, qualitative, scientific method, hypothesis, theory, control, variable, accuracy, precision, percent error

Measurements: mass, volume, length, density, time, energy

Base Units: gram, liter, meter, seconds, Joules

Metric System: M, K, H, D, d, c, m, μ, n

Dimensional Analysis: metric conversions, density

Scientific Notation

Calculator Usage: exponents, parenthesis

Ch3: Atomic Structure

Vocab: neutral, isotope, atomic number, atomic mass

Theories/Scientists: Atomic Theory/Dalton, Plum Pudding Model/Cathode Ray Tube/Thomson, Gold Foil Experiment/Rutherford, Solar System Model/Bohr, Electrons Cloud Model/Quantum Mechanical Model/Shrodinger

Subatomic Particles: proton, neutron, electron

Structure: nucleus, cloud

Ch4: Electrons in Atoms

Vocab: photon, frequency, wavelength, photoelectric effect, line emission spectrum, ground state, excited state

Formulas: c = λν and E = hν

Variables: ν = frequency (Hertz = cycle/sec = 1/sec = sec -1), λ = wavelength (1m = 100cm), energy (Joules)

Constants: c = speed of light = 3.00 x 108 m/s and h = Planck’s constant = 6.626 x 10 -34 J* s

Wave/Particle Duality of Motion: photoelectric effect, line emission spectra, electromagnetic radiation (which evidence supports waves or particles)

Scientists: Planck, Heisenberg, de Broglie, Einstein, Hund, Pauli

Electron Configurations: energy levels (n), sublevels (s,p,d,f), orbitals (1,3,5,7), electrons (2,6,10,14), the Aufbau Principle, Noble Gas Notation, maximum orbitals = n2, maximum electrons = 2n2

Ch5: Periodic Trends

Vocab: ionization energy, electronegativity, electron affinity, atomic radii, ionic radii, periodic law, valence electrons, cations, anions

Scientists: Mendeleev, Moseley

Ch6: Bonding

Vocab: ionic character, octet rule, Lewis structure, ion, malleable, ductile, lustrous

Compounds and their Properties: Ionic and Molecular

Bonds: Ionic, Covalent, Metallic

VSEPR: linear, bent, trigonal planar, trigonal pyramidal, tetrahedral

Polarity: nonpolar covalent bond, polar covalent bond, nonpolar molecule, polar molecule

Intermolecular Attractions (Forces): hydrogen bonds, dipole interactions, London dispersion forces

Ch21: Nuclear Chemistry

Vocab: nuclide, nucleon, radioisotope, decay/emission, absorption/capture, fission, fusion

Nuclear Stability: proton to neutron ratio

Radiation: alpha, beta, gamma, positron, proton, neutron

Half-lives

Study all your chapter notes and vocabulary!!

90. What is the formula for Lead (II) chromate? __________________Aluminum sulfate? __________________

91. Name the compounds: Ni(ClO3)2, ____________________Zn3(PO4)2, ___________________KClO3, _____________________ CF4,_______________ N2_,_______________ O4, _______________ SO3,_______________

92. What is the formula for: nitrogen trifluoride __________, sulfur dichloride ___________, nitrogen monoxide,_______________

93. When is a Roman numeral used in naming a compound? _______________________When is a prefix used? ________________

94. What is the molar mass of KClO3?

95. How mass in grams of 3.5 moles of KClO3?

96. How many molecules of the KClO3 are found in 3.5 x 108 grams of KClO3?

97. How many atoms of oxygen are in 5.05 x 102 g of KClO3 ?

98. What is the percentage of oxygen in SO2?

99. What is the percentage of Cu in CuCl2?

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