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 electronegativity

32. Circle the answer which makes the statements below true:

a. The strength of a covalent bond (increases/decreases) with increasing bond order. Therefore

(single/double/triple) bonds are the strongest.

b. The length of a covalent bond (increases/decreases) with increasing bond order. Therefore

(single/double/triple) bonds are the longest and (single/double/triple) bonds are the shortest.

33. Determine the number of valence electrons (VE) available and draw Lewis structures for the

following molecules:

a. SO3 VE = ____________ b. ClO3– VE = ____________

c. CH2O VE = ____________ d. BrF3 VE = ____________

34. For each of the following molecules below, give the (1) the molecular geometry geometry/shape

(2) state if it is a polar or nonpolar molecule

Molecule

Questions #1 – 3

a.

1) 2)

b.

1)

2)

c.

1) 2)