Name ______Date ______Period ______
Study Guide
1)Determine the number of significant digits in
900 - ______9004 - ______0.005016 - ______8.0400 - ______
2) Calculate the following measurements and round off using the correct number of significant digits.
3.4 cm x 10.9 cm x 0.92 cm = ______(103.45 g – 99.7 g) 7.43 mL = ______
3) Identify the following as an element, compound, hetero or homo mixture
a. Iron b. steel c. water d. sugar
e. air f. has atoms g. has identifiable parts h. contains molecules
i. kool-aid j. must combine atoms chemically
4) Which boxes contain: - one element - a compound - a mixture
5) Identify the following as chemical or physical changes.
a. melting ice b. burning rubber c. exploding fireworks
d. dissolving sugar e. boiling salt water
6) Give an example of a chemical and physical change that can occur to the following:
- Paper
- Salt
- Metal
7) Identify the four indicators of a chemical reaction.______, ______, ______, ______.
8) Which of the following statements are true about subatomic particles? Can be more than one!!
a) Protons and electrons can be found in the nucleus.
b) Electrons are found in orbitals around the nucleus
c) Neutrons are positively charged particles
d) Protons and electrons weigh the same
e) Isotopes of an element have different numbers of neutrons
f) Ions of an element have different numbers of protons
9) Determine the number of protons, neutrons and electrons in
A. Silicon – 29 p = ____ n = _____ e = ____ B. 24 Na p = ____ n = _____ e = ____
C. 35Cl p = ____ n = _____ e = ____ D. 36 Cl-2 p = ____ n = _____ e = ____
10) Consider the following % Abundances for these isotopes of Oxygen. Then calculate the average atomic mass for the sample:
Oxygen-15 (13.5%) Oxygen-16 (83.9%) Oxygen-18 (2.6%)
11) There are two isotopes of O: O-15 and O-16. Using Oxygen’s average atomic mass from the periodic table, explain which isotope is the most abundant and how you know.
12) Titanium has five common isotopes: 46Ti (8.0%), 47Ti (7.8%), 48Ti (73.4%), 49Ti (5.5%), 50Ti (5.3%). What is the average atomic mass of titanium?
13) The half-life for Fm-255 is 20.1 hours. How long will it take for a 32.0g sample to decay until only 2.00g remains?
14) Three grams of Bismuth-218 decay to 0.375 grams in one hour. What is the half-life of this isotope?
15) Actinium-226 has a half-life of 29 hours. If 100 mg of actinium-226 disintegrates over a period of 58 hours, how many mg of actinium-226 will remain?
16) Fill in the following nuclear decay equations:
5927 Co 4 2He + ______23892 U 23490Th + _____
21482Pb 0-1 + ______23490Th23491Pa + ______+ γ
17) Which section of the EM spectrum has the:
- Lowest energy?
- Shortest Wavelength?
- Smallest Frequency?
18) What wavelength of energy is released when an electron moves from:
a. 6 to 1 b. 5 to 3 c. 4 to 1 d. 4 to 2
19) What are the periodic table trends for:
Ionization Energy Activity or Reactivity Atomic Radius Electronegativity
20) This picture could represent which of the following?
a. Iron b. Potassium c. Silver d. Carbon e. Argon f. Barium
21) Write the orbital notation for
a. Li b. Si c. Na d. F
22) Determine the element represented below
a. 1s22s22p63s23p64s23d6 b. 1s22s22p4 c. [Kr]5s24d3
d. [Rn]7s2 e. [Xe] 6s24f145d7
23) Draw the electron dot structures for the following elements:
a. Rb b. Ba c.Cl d.As e. B f. Cr
24) Which element is in Group 3& Period 6 of the periodic table?
25) Which element in Group 16 has the least tendency to gain electrons?
26) Within each of the following groups, state which has the largest ionization energy:
a. Mg and Be b. As and Se c. Fr and Ba d.Cl and Ar
27) Within each of the following groups, state which has the greatest electronegativity:
a. Na and Mg b. C and Si c. Ge and P d.Cl and Ar
28) Rank the following from least to most reactive:
a. Ba, Fe, Y b. S, Se, I c. F, Cl, Br d. Na, K, Rb
29) For each of the following compounds, determine if it is ionic or covalent and draw the dot diagram. If it is covalent, identify the shape, overall polarity, and intermolecular forces present:
a. NH3
b. PF3
c. KF
d. CH4
e. HF
f. Li2O
g. H2O
h. CO2
30) Fill out the following table:
Type of bond / Does it dissolve? / Does it conduct electricity?Metallic
Ionic
Polar Covalent
Non-Polar Covalent
32) Write the formulas for the substances:
a. magnesium carbonate b. iron (II) hydroxide c. silicon disulfide
d. silver nitride e. lean (III) chloride f.heptanitrogen trichloride
33) Name the following substances
a. N2O b. SiF4 c. K2SO4
d. Mn(C2H3O2)2 e. C4F5 f. FeO2
34) Determine the molar (formula) mass of
a.Al(C2H3O2)3 b. Cr(OH)3 c. MnF
35) Convert 915 g of SiBr4 to molecules.
36) How many moles in 8.2 x 10 21 atoms of Xe?
37) How many grams are in 3.9 x 1025 atoms of Ba?
38) Determine the number of moles in 250 g of CO2.
39) Calculate the % composition of O in the following
a. P2O5 b. MgSO4 c. Fe3(PO4)2
40) What is the empirical formula for a compound which contains 0.0134 g of iron, 0.00769 g ofsulfur and 0.0115 g of oxygen?
41) What’s the empirical formula of a molecule containing 65.5% carbon, 5.5% hydrogen, and 29.0% oxygen?
42) What is the molecular formula of a compound that is 0.606 g of N and 1.29 g of O if the mass is 92g?
43) What is the molecular formula if the empirical is CH2 and the molecular molar mass is 70g?
List properties of the following:
Metals –
Nonmetals –
Endothermic Reactions –
Exothermic Reactions –
Define the following:
Ionization Energy –
Electronegativity –
Ionic Bond –
Covalent Bond –
Metallic Bond –
Polar –
Nonpolar –
Lewis Structure –
Valence Electron –
Isotope –
Ion –