Honors Chemistry Midterm: Review Packet Honors Chemistry Name: _____ Date: _____ Mods: _____ Honors

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  • Honors Chemistry

    Name: ______________________________________ Date: ________________ Mods: ____________

    Honors Chemistry Midterm: Review Packet

    1. Write in the number of significant figures for each of the following measurements:

    ____ 3.00 mL ___ 0.00290 g ___ 50.00 m ___ 0.070 kg ___ 400 L

    2. Using the following masses: 0.0562 kg, 124.213 g and 1635 mg. The answer should be reported as: ______________ g

    3. a) A 5.75 mL sample of mercury has a measured mass of 77.05 g. The density is ___________.

    b) Mercury’s accepted density is 13.53 g/mL. The % error in your measurement is: __________.

    4. In the diagram below:

    Is this person accurate? ___________

    Is this person precise? ___________

    5. Identify the following as a chemical change (CC), physical change (PC), chemical property (CP), or physical property (PP):

    a) burning wood __________ b) mass of wood _________

    c) flammability of wood _________ d) chopping up wood __________

  • 6. A calculator displays the answer to a problem as 53.09010 Report this answer to:

    _______________________ 5 significant figures

    _______________________ 3 significant figures

    _______________________ 1 significant figure

    7. a) What is an isotope?

    b) Calculate the average atomic mass of silicon. The three silicon isotopes have atomic masses and relative abundances of 27.9769 amu (92.2297%), 28.9765 amu (4.6832%) and 29.9738 amu (3.0872%).

    8. a) Who is the scientist responsible for the discovery of the electron?

    b) What was the experiment that led to this discovery?

    9. Write the formulas for the following ionic and molecular compounds:

    Name Formula

    tin (IV) chloride

    Tetracarbon diphosphide

    aluminum hydroxide

    ammonium sulfate

    nitrogen tribromide

    calcium phosphate

  • 10. Write the names of the following ionic and molecular compounds

    Name Formula

    Pb3(PO4)2

    KMnO4

    O2F5

    ZnSO4

    MgO

    PSe2

    11. a) The molar mass of Ba(NO3)2 is ________________________________.

    b) Calculate the percent composition of each element in Ba(NO3)2

    Ba = ____________% N = ___________% O = ___________ %

    12. How many particles of CO2 (MM = 44.0 g/mol) are in 17.75 grams of CO2?

    13. List the seven diatomic molecules. (The ones that always come in pairs)

  • 14. Balance the following chemical equations and classify their type (single replacement, double replacement, etc.)

    a) _____C5H12 + _____O2  _____CO2 + _____H2O

    Classify this reaction: ______________________________________________________

    b) _____H2O2  _____H2O + ______O2

    Classify this reaction: ______________________________________________________

    c) _____AgNO3 + _____K2CO3  _____Ag2CO3 + _____KNO3

    Classify this reaction: ______________________________________________________

    15. Consider the balanced equation: N2(g) + 3 H2(g)  2 NH3(g)

    molar masses (g/mol): (28.0) (2.0) (17.0)

    a) What is the greatest mass of ammonia, NH3 (g), that will be formed when 12.80 grams of

    H2(g) reacts with 55.25 grams of N2(g)? (Hint: this is a limiting reactant problem)

    b) If this reaction was completed in the lab and it was determined that the quantity of ammonia

    gas produced was 63.4 grams, what is the % yield of the ammonia?

    16. A substance is 33.33% carbon, 7.47% hydrogen, and 59.20% oxygen.

    a) What is its empirical formula?

    b) If the molar mass of the compound is 216 g/mol, what is its molecular formula?

  • 17. In the following, circle the precipitates:

    PbI2 Ba(OH)2 Ag2CO3 CaF2 K2SO3 (NH4)2S

    18. Write the balanced molecular, complete ionic, and net ionic equation for the following:

    a) Solutions of magnesium chloride and lead (II) acetate are mixed.

    b) Solutions of silver nitrate and sodium carbonate are mixed.

  • 19. Write the balanced molecular equations.

    a) ______Co(C2H3O2)2 (aq) + ______Ag (s) _______________________________________

    b) ______Na (s) + ______AlCl3(aq) ______________________________________________

    c) ______H2SO4(aq) + ______Ca (s) _____________________________________________

    d) ______Br2(s) + ______CuI2(aq) ______________________________________________

    20. Fill in the blanks:

    a. The symbol for wavelength is ________ and it is measured in ________ or ________.

    b. The symbol for frequency is ________ and it is measured in ________ = ________.

    c. The speed of light, c, is a constant value of __________________________________.

    d. Planck’s constant, h, is a constant value of __________________________________.

    e. The equation relating wavelength and frequency is: ___________________________.

    f. The equation relating energy and frequency is: _______________________________.

    g. 1 nm = __________________________ m

    21. Rank the following in order from lowest (1) to highest (7)energy:

    gamma rays, visible light, microwaves, ultraviolet radiation, x-rays, radio waves, infrared radiation

    1) ___________________________________ 2) _____________________________________

    3) ___________________________________ 4) _____________________________________

    5) ___________________________________ 6) _____________________________________

    7) ___________________________________

  • 22. A certain photon of light has a frequency of 4.59 x 1014 Hz. Calculate the wavelength, in nanometers, of the light.

    23. A wave of blue light has a wavelength of 422 nm. What is the energy, in J, of that wave?

    24. Scientists and Energy:

    Matching – match the letter of the scientist to the work that he contributed to the world

    a) Heisenberg b) Louis de Broglie c) Niels Bohr d) Rydberg

    _________ responsible for the uncertainty principle which states that it is impossible to know

    (with any great degree of certainty) both the location and velocity of an electron)

    _________ responsible for the planetary model of the atom, where electrons traveled in

    distinct paths around the nucleus

    _________ responsible for the equation which determines the exact amount of energy

    needed for electron promotion or demotion between energy levels

    _________ responsible for the idea that if light can behave as particles of matter, matter

    should also be able to exhibit wave properties.

    25. Identify the elements with the following electron configurations:

    a. ___________________________ 1s22s22p63s23p64s23d104p6

    b. ___________________________ [Ar] 4s23d10

    c. ___________________________ [Ne] 3s2 3p4

    d. ___________________________ 1s22s22p63s23p64s23d104p65s24d2

    26. Which six elements are exceptions because they have unusual/irregular electron configurations?

  • 27. Write the condensed (noble gas) electron configuration for the following elements:

    a. Tin _________________________________________________________

    b. Osmium _________________________________________________________

    c. Chromium _________________________________________________________

    28. Periodic Trends:

    Matching – match the letter of the trend that is best described by the statements below

    a) atomic radius b) ionization energy c) electronegativity d) electron affinity

    _________ the energy required to remove an electron from an atom or ion

    _________ the energy change associated with an atom or ion gaining and electron

    _________ the relative size of an atom

    _________ the ability of an atom to attract electrons to itself

    29. Complete the diagram to the

    right by writing increase or

    decrease along the period and

    group arrows for each of the

    periodic trend.(AR = atomic

    radius, EN = electronegativity,

    IE = ionization energy)

    30. Use the following elements to

    answer the questions below

    (Note: an element can be used more than once):

    Tellurium, Chlorine, Selenium

    a. ____________________________ has the lowest 1st ionization energy

    b. ____________________________ has the highest 1st ionization energy

    c. ____________________________ is the largest atom

    d. ____________________________ has the highest electronegativity

  • 31. Use the following elements to answer the questions below (Note: an element can be used more

    than once):

    Aluminum, Beryllium, Nitrogen

    a. ____________________________ has the lowest 1st ionization energy

    b. ____________________________ is the smallest atom

    c. ____________________________ has the highest electronegativity

    d. ____________________________ has the lowest electroneg