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Name: _________________________________________ Date: __________ Period: ______
Atoms (textbook pages 258 – 279)
Chapter 10, Section 2 Review Questions
1. An atom’s ______________________ is equal to the number of protons in its nucleus
2. An atom’s ______________________ is equal to the weighted average of the masses of all the
naturally occurring isotopes of that element.
3. Which particle has no electric charge? ______________________
4. Name and describe the 4 forces that are at work within the nucleus of the atom:
a.
b.
c.
d.
5. Why is gravitational force in the nucleus so small?
6. Could a nucleus have more than one proton but no neutrons? Explain.
7. Look at the two atomic models below. Do the two atoms represent different elements or
different isotopes? Explain.
Periodic Table (textbook pages 282 – 305)
Chapter 11 Review Questions
Fill in the Blank
group
period
alkali metals
halogens
noble gases
alkaline-earth metals
8. Elements in the same vertical column on the periodic table belong to the same _____________.
9. Elements in the same horizontal row on the periodic table belong to the same ______________.
10. The most reactive metals are _______________________.
11. Elements that are unreactive are called ____________________.
Multiple Choice
12. _____ Mendeleev’s periodic table was useful because it…
a. Showed the elements arranged by atomic number
b. Had no empty spaces
c. Showed the atomic number of the elements
d. Allowed for the prediction of the properties of missing elements
13. _____ Most nonmetals are…
a. Shiny
b. Poor conductors of electric current
c. Flattened when hit with a hammer
d. Solids at room temperature
14. _____ Which of the following items is NOT found on the periodic table?
a. The atomic number of each element
b. The name of each element
c. The date that each element was discovered
d. The atomic mass of each element
15. _____ Which of the following statements about the periodic table is false?
a. There are more metals that nonmentals on the periodic table
b. Atoms of elements in the same group have the same number of electrons in the outer
level
c. The elements at the far left of the periodic table are nonmetals
d. Elements are arranged by increasing atomic number
16. _____ Which of the following statements about alkali metals is true?
a. Alkali metals are generally found in their uncombined form
b. Alkali metals are group 1 elements
c. Alkali metals should be stored underwater
d. Alkali metals are unreactive
17. _____ Which of the following statements about elements is true?
a. Every element occurs naturally
b. All elements are found in their uncombined form in nature
c. Each element has a unique atomic number
d. All of the elements exist in approximately equal quantities
Chemical Bonding (textbook pages 308 – 329)
Chapter 12 Review Questions
Fill in the Blank
Crystal lattice
molecule
chemical bonding
Covalent bond
ionic bond
metallic bond
valence electron
chemical bond
ion
18. An interaction that holds two atoms together is a(n) ____________________________.
19. A charged particle that forms when an atom transfers electrons is a(n) ____________________.
20. A bond formed when atoms share electrons is a(n) __________________________.
21. An electron in the outermost energy level of an atom is called a(n) _______________________.
22. Ionic compounds are bonded in a three-dimensional pattern called a(n)
________________________________.
Multiple Choice
23. _____ Which element has a full outermost energy level containing only two electrons?
a. Fluorine, F
b. Helium, He
c. Hydrogen, H
d. Oxygen, O
24. _____ Which of the following describes what happens when an atom becomes an ion with a 2charge?
a. The atom gains 2 protons
b. The atom loses 2 protons
c. The atom gains 2 electrons
d. The atom loses 2 electrons
25. _____ The properties of ductility and malleability are associated with which type of bonds?
a. Ionic
b. Covalent
c. Metallic
d. All of the above
26. _____ What type of element tends to lose electrons when it forms bonds?
a. Metal
b. Metalloid
c. Nonmetal
d. All of the above
27. _____ Which pair of electrons can form an ionic bond?
a. Sodium, Na & potassium, K
b. Potassium, K & fluorine, F
c. Fluorine, F & chlorine, Cl
d. Sodium, Na & neon Ne
Short Answer
28. List 2 properties of covalent bonds
29. Explain why an iron ion is attracted to sulfide but not a zinc ion.
30. Compare the 3 types of bonds based on what happens to the valence electrons of the atoms.
Chemical Reactions (textbook pages 332 – 343)
Chapter 13, Sections 1 and 2 Review Questions
31. _____ Most chemical reactions….
a. Result in substances that have different properties
b. Do not break bonds
c. Do not rearrange atoms
d. Have no effects that can be seen
32. Steam is escaping from a teapot. Is this a chemical or physical change? Explain.
33. _____ The correct formula for carbon tetrachloride is….
a. CCL3
b. C3Cl
c. CCL
d. CCL4
34. _____ Calcium oxide is used to make soil less acidic. Its formula is….
a. CA2O2
b. CAO
c. CAO2
d. CA2O
35. Balance the following equations by adding the correct coefficient:
a. Na
+
Cl2

NaCl
b.
Mg
+

N2
Mg3N2
36. How does a balanced equation illustrate that mass is never lost or gained in a chemical reaction?
37. Circle the reactants and put a square around the products in the following equation:
C
+
O2

CO2
T-CAP Ready
38. _____ Based on their locations on the Periodic Table, which two elements share the MOST
similar chemical properties?
a.
b.
c.
d.
K & Kr
Be & Ba
S & Sn
H&I
39. _____ In what order are the regions arranged on the periodic table, reading from left to right.
a. Inert gases, metals, nonmetals, metalloids
b. Metalloids, metals, nonmetals, inert gases
c. Metals, metalloids, nonmetals, inert gases
d. Nonmetals, inert gases, metals, metalloids
40. _____ How are the elements arranged in the periodic table?
a. By their atomic mass
b. By their chemical symbol
c. By their chemical name
d. By their atomic number
41. _____ According to its location on the periodic table, sodium can be described as…
a. An alkaline-earth metal
b. A transition metal
c. An alkali metal
d. A metalloid