1. Chapters 11 & 12 Review

2. Which of the following determines the identity of an element?
A. Atomic Number C. Atomic Mass
B. Mass Number D. Overall Charge
Isotopes exist because atoms of the same element can have different numbers of
A. Protons C. Electrons
B. Neutrons D. None of the Above

3. An atom’s structure determines its properties
An atom’s structure determines its properties. What property of an atom is affected by the difference between the number of its protons and the number of its electrons?
A. Atomic number C. Size
B. Atomic mass D. Charge

4. The black circles in the model above represent neutrons
The black circles in the model above represent neutrons. What do the white circles represent?
A. Electrons C. Nuclei
B. Isotopes D. Protons

5. Which of the following about the periodic table is false?
A. There are more metals than nonmetals on the periodic table.
B. Atoms of elements in the same group have the same number of electrons in their outer level.
C. The elements at the far left of the periodic table are nonmetals.
D. Elements are arranged by increasing atomic number.

6. 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.

7. What nonmetal is in the same group as Lead?
A. Tin B. Nitrogen
C. Carbon D. Silicon
Fluorine, Chlorine, Bromine, Iodine, and Astatine make up Group 17, the Halogens. Why are these elements grouped together?
A. They are all very reactive nonmetals with similar chemical properties.
B. They are all nonreactive gases.
C. Their atoms have8 valence electrons.
D. They all have the same atomic number.

8. Which of these does the number of electrons in the outer level indicate about the element?
A. Its reactivity C. Its atomic number
B. Its mass number D. Its symbol
Which element has a full outermost energy level containing only two electrons?
A. Fluorine C. Hydrogen
B. Helium D. Oxygen

9. 11. Which of the following describes what happens when an atom becomes an ion with a 2- charge?
A. The atom gains 2 protons.
B. The atom loses 2 protons.
C. The atom gains 2 electrons.
D. The atom loses 2 electrons.

10. What type of element tends to lose electrons when it forms bonds?
A. Metal C. Nonmetal
B. Metalloid D. Noble gas
Which pair of atoms can form an ionic bond?
A. Sodium and Potassium
B. Potassium and Fluorine
C. Fluorine and Chlorine
D. Sodium and Neon

11. For each atom below, write the number of electrons it must gain or lose to have 8 valence electrons. Then, calculate the charge of the ion that would form.
Calcium
Phosphorus
Bromine
Sulfur

12. Predict the type of bond each of the following pairs of atoms would form:
Oxygen and Nitrogen
Magnesium and Chlorine

13. Look at the picture above
Look at the picture above. To make the atom have a full energy level, _____ electrons need to be added.
A. 5 C. 8
B. 3 D. 0

14. For the test…
I can determine the number of protons, neutrons, and electrons in an atom.
I can identify the group names on the periodic table.
I can determine the most reactive elements on the periodic table.
I can predict what elements will form ionic bonds and covalent bonds.
I can analyze electron-dot diagrams.
I can determine which elements will lose electrons and which elements will gain electrons.