14. which element would most likely form +2 ions?
a. sodium
b. magnesium
c. chlorine
d. neon
15. which element has 4 valence electrons?
a. boron
b. carbon
c. nitrogen
d. oxygen
16. which element is a metalloid and a semiconductor?
a. oxygen
b. silicon
c. iron
d. sodium
17. which elements are most likely brittle and dull?
a. metals
b. metalloids
c. nonmetals
d. noble gases
18. which group contains the most reactive nonmetals?
a. 1
b. 2
c. 16
d. 17
19. which element is used in neon signs?
a. helium
b. neon
c. argon
d. krypton
20. which group contains the transition metals?
a. 1–2
b. 13–18
c. 3–12
d. 16–18
21. which is not a property of metals?
a. conductive
b. malleable
c. brittle
d. shiny
22. where are metalloids found?
a. far right
b. far left
c. along the zig - zag line
d. in the noble gases
23. which element is a nonmetal but is in group 1?
a. lithium
b. hydrogen
c. sodium
d. potassium
24. which family contains oxygen and sulfur?
a. halogens
b. noble gases
c. chalcogens
d. alkali metals
25. which particle determines the identity of an element?
a. electron
b. neutron
c. proton
d. valence electron
bonding & formulas (26–45)
26. a sodium atom loses one electron. what is formed?
a. neutral atom
b. anion
c. cation
d. isotope
27. when a metal and nonmetal bond, what type of bond forms?
a. covalent
b. metallic
c. hydrogen
d. ionic

Question

Accepted Answer

### Question 14
# Brief Explanations:
To determine which element forms +2 ions, we analyze each option:
- Sodium (Na) is in Group 1, so it loses 1 electron to form $ \text{Na}^+ $ (not +2).
- Magnesium (Mg) is in Group 2, so it loses 2 electrons to form $ \text{Mg}^{2+} $.
- Chlorine (Cl) is a nonmetal in Group 17, it gains 1 electron to form $ \text{Cl}^- $ (not +2).
- Neon (Ne) is a noble gas, it does not form ions easily.
So Magnesium is the correct choice.
# Answer:
B. Magnesium

### Question 15
# Brief Explanations:
Valence electrons are determined by the group number (for main - group elements).
- Boron (B) is in Group 13, so it has 3 valence electrons.
- Carbon (C) is in Group 14, so it has 4 valence electrons.
- Nitrogen (N) is in Group 15, so it has 5 valence electrons.
- Oxygen (O) is in Group 16, so it has 6 valence electrons.
Thus, Carbon has 4 valence electrons.
# Answer:
B. Carbon

### Question 16
# Brief Explanations:
We analyze each option to find the metalloid and semiconductor:
- Oxygen (O) is a nonmetal, not a metalloid.
- Silicon (Si) is a metalloid and is widely used as a semiconductor.
- Iron (Fe) is a metal, not a metalloid.
- Sodium (Na) is a metal, not a metalloid.
So Silicon is the correct answer.
# Answer:
B. Silicon

### Question 17
# Brief Explanations:
We recall the properties of different element types:
- Metals are generally malleable, ductile, and shiny.
- Metalloids have properties intermediate between metals and nonmetals.
- Nonmetals are often brittle and dull (except for some like graphite).
- Noble gases are a type of nonmetal, but the question asks for the general category of brittle and dull elements, and nonmetals (excluding noble gases in terms of this property description) are brittle and dull.
So nonmetals are the ones that are most likely brittle and dull.
# Answer:
C. Nonmetals

### Question 18
# Brief Explanations:
The reactivity of nonmetals:
- Group 1 elements are metals (alkali metals), very reactive but they are metals.
- Group 2 elements are alkaline earth metals (metals).
- Group 16 elements are chalcogens (nonmetals/metalloids), not the most reactive nonmetals.
- Group 17 elements are halogens (nonmetals). Halogens are the most reactive nonmetals because they need to gain only 1 electron to achieve a stable octet configuration.
So Group 17 contains the most reactive nonmetals.
# Answer:
D. 17

### Question 19
# Brief Explanations:
Neon signs use neon gas. Helium is used in balloons and some lighting, argon is used in welding and some lighting, and krypton is used in some lighting applications but neon is specifically used in neon signs.
# Answer:
B. Neon

### Question 20
# Brief Explanations:
The location of transition metals in the periodic table:
- Groups 1 - 2 are the alkali and alkaline earth metals (main - group metals).
- Groups 13 - 18 are the main - group elements (including metalloids, nonmetals, and some metals).
- Groups 3 - 12 are the transition metals.
- Groups 16 - 18 include chalcogens, halogens, and noble gases.
So transition metals are in Groups 3 - 12.
# Answer:
C. 3 - 12

### Question 21
# Brief Explanations:
Properties of metals:
- Metals are conductive (they can conduct heat and electricity).
- Metals are malleable (they can be hammered into shapes).
- Metals are shiny (have a metallic luster).
- Brittle is a property of nonmetals (and some metalloids), not metals.
So brittle is not a property of metals.
# Answer:
C. Brittle

### Question 22
# Brief Explanations:
Location of metalloids in the periodic table:
- The far right of the periodic table has nonmetals.
- The far left has metals (alkali and alkaline earth metals).
- Metalloids are found along the zig - zag line that separates metals and nonmetals in the periodic table.
- Noble gases are in Group 18 (far right), they are nonmetals, not metalloids.
So metalloids are found along the zig - zag line.
# Answer:
C. Along the zig - zag line

### Question 23
# Brief Explanations:
We analyze each option:
- Lithium (Li) is a metal in Group 1.
- Hydrogen (H) is a nonmetal and it is in Group 1.
- Sodium (Na) is a metal in Group 1.
- Potassium (K) is a metal in Group 1.
So Hydrogen is a nonmetal in Group 1.
# Answer:
B. Hydrogen

### Question 24
# Brief Explanations:
The family of oxygen and sulfur:
- Halogens are Group 17 elements (e.g., fluorine, chlorine).
- Noble gases are Group 18 elements (e.g., helium, neon).
- Chalcogens are Group 16 elements, and oxygen (O) and sulfur (S) are in Group 16, so they belong to the chalcogen family.
- Alkali metals are Group 1 elements (e.g., lithium, sodium).
So oxygen and sulfur belong to the chalcogens family.
# Answer:
C. Chalcogens

### Question 25
# Brief Explanations:
The particle that determines the identity of an element:
- Electrons are involved in chemical reactions, but the number of electrons can change (forming ions).
- Neutrons are part of the nucleus, but changing the number of neutrons forms isotopes (same element, different mass).
- Protons: The number of protons in an atom's nucleus is the atomic number, and each element has a unique atomic number (number of protons). So the number of protons determines the identity of an element.
- Valence electrons determine the chemical properties, not the identity.
So protons determine the identity of an element.
# Answer:
C. Proton

### Question 26
# Brief Explanations:
When a sodium atom loses an electron:
- A neutral atom has an equal number of protons and electrons.
- An anion is formed when an atom gains electrons (has more electrons than protons).
- A cation is formed when an atom loses electrons (has more protons than electrons). Sodium (Na) has 11 protons and 11 electrons. When it loses 1 electron, it has 11 protons and 10 electrons, so it has a positive charge ($ \text{Na}^+ $), which is a cation.
- Isotopes are atoms of the same element with different numbers of neutrons, not related to electron loss/gain in this context.
So a sodium atom losing one electron forms a cation.
# Answer:
C. Cation

### Question 27
# Brief Explanations:
Type of bond between a metal and a nonmetal:
- Covalent bonds are formed between two nonmetals (sharing of electrons).
- Metallic bonds are formed between metal atoms (sea of delocalized electrons).
- Hydrogen bonds are a type of intermolecular force, not a primary bond type between a metal and nonmetal.
- Ionic bonds are formed between a metal (which loses electrons to form a cation) and a nonmetal (which gains electrons to form an anion). The electrostatic attraction between the cation and anion forms an ionic bond.
So when a metal and nonmetal bond, an ionic bond forms.
# Answer:
D. Ionic

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