NAME __________________________________________ PERIOD ______SAGE INTERIM Review
1. Which particle is correctly matched to its charge?
a. Electron; no charge
c. Proton; no charge
b. Neutron, negative charge
d. Proton; positive charge
2. Which particles make up the nucleus?
a. Electrons and protons
b. Electrons and neutrons
c. Protons and neutrons
d. Protons only
3. In chemistry, what does an “amu” measure?
a. The mass of an atom
b. The radius of an atom
c. The charge of an atom
d. The velocity of an atom
4. Which is true of electrons in larger orbitals?
a. They have less charge
b. They have less energy
c. They have more charge
d. They have more energy
5. Which is true of atomic structure?
a. Electrons orbit the nucleus in clouds
b. Electrons orbit the nucleus in defined paths
c. Protons orbit the nucleus in clouds
d. Protons orbit the nucleus in defined paths
6. Use standard notation to represent sodium. Give the number of protons, neutrons, and
electrons in the element.
7. An atom has 2 electrons, 3 protons, and 4 neutrons. What is the atomic mass?
a. 3
b. 5
c. 7
d. 9
8. The atomic number is equal to the number of ________
9. An atom with 6 protons, 6 neutrons, and 6 electrons has a mass of approximately ___
a. 6 amu
c. 18 amu
b. 12 amu
d. 36 amu
10. Given 𝟓𝟕
𝟐𝟔𝑭𝒆 , determine the mass number.
11. If an atom has 19 electrons, 20 neutrons, and an atomic mass of 39, how many protons
are in the nucleus?
12. If a gold atom has 79 protons and 118 neutrons, what is the standard notation?
𝟕𝟗
a. 𝟏𝟗𝟕
𝑨𝒖
b. 𝟏𝟏𝟖
𝟕𝟗𝑨𝒖
c. 𝟏𝟗𝟕
𝟗𝟕𝑨𝒖
13. Which particle is a negatively charged ion?
a. Hydrogen with 1 proton, 0 neutrons, and 1 electron
b. Sodium with 11 protons, 12 neutrons, and 10 electrons
c. Chlorine with 17 protons, 18 neutrons, and 18 electrons
d. Magnesium with 12 protons, 12 neutrons, and 12 electrons
14. What is the number of each subatomic particle in a carbon 12 atom?
Protons:__________ Neutrons:__________ Electrons: __________
d. 𝟏𝟗𝟕
𝟏𝟏𝟖𝑨𝒖
15. Which of the following is true for chemical compounds that have been detected
elsewhere in the universe?
a. They have a greater average density than the same compounds found on Earth
b. They are composed of the same elements that are found on Earth
c. They are less reactive chemically than the same compounds found on Earth.
d. Those with the greatest atomic masses are found furthest away from our solar
system.
16. Which of the following is an example of a covalent compound?
a. Aluminum oxide (Al2O3)
b. Calcium phosphate (Ca3(PO4)2)
c. Hydrogen chloride (HCl)
d. Sodium chloride (NaCl)
17. Which of the following is an example of an ionic compound?
a. Carbon dioxide (CO2)
c. Silver nitrate (AgNO3)
b. Hydrochloric acid (HCl)
d. Water (H2O)
18. Magnesium (Mg) belongs to group 2 of the periodic table. Which elements will
magnesium form an ionic bond with?
a. Fluorine only
b. Fluorine and oxygen
c. Fluorine, oxygen, and sodium
d. Fluorine, oxygen, sodium and calcium
19. At room temperature, some compounds are gases, some are liquids, and some are solids.
Which of the following classes of compounds exhibits this variety of phases?
a. Covalent compounds
c. Metallic compounds
b. Ionic compounds
d. Network covalent compounds
20. Identify these changes as physical or chemical.
a. Frying an egg
b. Heating metal until it changes color
c. Melting ice
d. Metal reacting with acid, producing hydrogen gas
21. For the element
238
92𝑈,
write the symbol for the isotope with 3 fewer neutrons.
22. Which of the following is evidence that a chemical reaction has occurred?
a. A liquid boils
c. The chemicals change colors
b. The reactants get smaller
d. The reactants have a strong odor
23. Why do sodium and chlorine combine to form sodium chloride?
a. Both sodium and chlorine atoms gains electrons to become stable
b. Both sodium and chlorine atoms lose electrons to become stable
c. Sodium atoms gain electrons and chlorine atoms lose electrons to become stable.
24. Which of the following statements about ionic and covalent compounds would you use as
evidence to explain the high melting and boiling points of ionic compounds?
a. Ions are held together by strong electrostatic forces.
b. Two or more nonmetal ions share valence electrons in a bond.
c. Atoms are held together by the shared attraction of valence electrons.
d. Metal cations bond to nonmetal anions by a transfer of valence electrons
25. What is the correct formula for aluminum oxide?
26. Use S-33 to determine the following.
a. # of protons
b. # of neutrons
c. # of electrons
27. What describes the bonds between atoms in an iron nail?
a. Polar covalent bonds
b. Ionic bonds
c. Metallic bonds
28. Which of the following is NOT a property of metals
a. Brittleness
b. Conductivity
c. Ductility
d. malleability
29. What property of metals makes them ideal for creating cooking pots?
a. Ductility
b. High melting point
c. Luster
d. malleability