Unit 2 Review

Titanium, atomic #22, belongs to the
1. Halogens
2. Alkali metals
3. Noble gases
4. Transition metals
5. Alkaline earth metals
6. Nonmetals
7. Semi-metals (metalloids)
Potassium, atomic #19, belongs to the
1. Halogens
2. Alkali metals
3. Noble gases
4. Transition metals
5. Alkaline earth metals
6. Nonmetals
7. Semi-metals (metalloids)
Xenon, atomic #54, belongs to the
1. Halogens
2. Alkali metals
3. Noble gases
4. Transition metals
5. Alkaline earth metals
6. Nonmetals
7. Semi-metals (metalloids)
Beryllium, atomic #4, belongs to the
1. Halogens
2. Alkali metals
3. Noble gases
4. Transition metals
5. Alkaline earth metals
6. Nonmetals
7. Semi-metals (metalloids)
Gold, atomic #79, belongs to the
1. Halogens
2. Alkali metals
3. Noble gases
4. Transition metals
5. Alkaline earth metals
6. Nonmetals
7. Semi-metals (metalloids)
Phosphorus, atomic #15, belongs to the
1. Halogens
2. Alkali metals
3. Noble gases
4. Transition metals
5. Alkaline earth metals
6. Nonmetals
7. Semi-metals (metalloids)
Germanium, atomic #32, belongs to the
1. Halogens
2. Alkali metals
3. Noble gases
4. Transition metals
5. Alkaline earth metals
6. Nonmetals
7. Semi-metals (metalloids)
Iodine, atomic #53, belongs to the
1. Halogens
2. Alkali metals
3. Noble gases
4. Transition metals
5. Alkaline earth metals
6. Nonmetals
7. Semi-metals (metalloids)
Nickel, atomic #28, belongs to the
1. Halogens
2. Alkali metals
3. Noble gases
4. Transition metals
5. Alkaline earth metals
6. Nonmetals
7. Semi-metals (metalloids)
Cesium, atomic #55, belongs to the
1. Halogens
2. Alkali metals
3. Noble gases
4. Transition metals
5. Alkaline earth metals
6. Nonmetals
7. Semi-metals (metalloids)
Argon, atomic #18, belongs to the
1. Halogens
2. Alkali metals
3. Noble gases
4. Transition metals
5. Alkaline earth metals
6. Nonmetals
7. Semi-metals (metalloids)
Strontium, atomic #38, belongs to the
1. Halogens
2. Alkali metals
3. Noble gases
4. Transition metals
5. Alkaline earth metals
6. Nonmetals
7. Semi-metals (metalloids)
Carbon, atomic #6, belongs to the
1. Halogens
2. Alkali metals
3. Noble gases
4. Transition metals
5. Alkaline earth metals
6. Nonmetals
7. Semi-metals (metalloids)
Antimony, atomic #51, belongs to the
1. Halogens
2. Alkali metals
3. Noble gases
4. Transition metals
5. Alkaline earth metals
6. Nonmetals
7. Semi-metals (metalloids)
Iridium, atomic #77, belongs to the
1. Halogens
2. Alkali metals
3. Noble gases
4. Transition metals
5. Alkaline earth metals
6. Nonmetals
7. Semi-metals (metalloids)
Hydrogen, atomic #1, belongs to the
1. Halogens
2. Alkali metals
3. Noble gases
4. Transition metals
5. Alkaline earth metals
6. Nonmetals
7. Semi-metals (metalloids)
Mercury, atomic #80, belongs to the
1. Halogens
2. Alkali metals
3. Noble gases
4. Transition metals
5. Alkaline earth metals
6. Nonmetals
7. Semi-metals (metalloids)
Arsenic, atomic #33, belongs to the
1. Halogens
2. Alkali metals
3. Noble gases
4. Transition metals
5. Alkaline earth metals
6. Nonmetals
7. Semi-metals (metalloids)
Neon, atomic #10, belongs to the
1. Halogens
2. Alkali metals
3. Noble gases
4. Transition metals
5. Alkaline earth metals
6. Nonmetals
7. Semi-metals (metalloids)
Sulfur, atomic #16, belongs to the
1. Halogens
2. Alkali metals
3. Noble gases
4. Transition metals
5. Alkaline earth metals
6. Nonmetals
7. Semi-metals (metalloids)
Generally speaking, the group of elements least likely to form ions are:
1. Group 1 - the alkali metals
2. Group 16 - the oxygen family
3. Group 17 - the halogens
4. Group 18 - the Noble gases
The most active metals are located in the:
1. lower right hand corner of the periodic table
2. lower left hand corner of the periodic table
3. upper right hand corner of the periodic table
4. upper left hand corner of the periodic table
Given the representation of a chlorine atom, which circle might represent an atom of fluorine?
1. None of these
2. Circle B
3. Circle C
4. Circle D
Given the representation of a chlorine atom, which circle might represent an atom of bromine?
1. None of these
2. Circle B
3. Circle C
4. Circle D
Given the representation of a chlorine atom, which circle might a chloride ion, Cl^-?
1. None of these
2. Circle B
3. Circle C
4. Circle D
Cations have a ______________ charge and are ______________ than the atoms from which they formed.
1. positive/larger
2. positive/smaller
3. negative/larger
4. negative/smaller
Anions have a ______________ charge and are ______________ than the atoms from which they formed.
1. positive/larger
2. positive/smaller
3. negative/larger
4. negative/smaller
As one moves down ( ↓ ) a group on the periodic table, the atomic radius of the elements encountered:
1. increases
2. decreases
3. stays the same
Of the following elements, which one would have the largest radius?
1. Hydrogen (H, atomic #1)
2. Sodium (Na, atomic #11)
3. Potassium (K, atomic #19)
4. Cesium (Cs, atomic #55)
Of the following elements, which one would have the smallest radius?
1. Fluorine (F, atomic #9)
2. Chlorine (Cl, atomic #17)
3. Bromine (Br, atomic #35)
4. Iodine (I, atomic #53)
Which of the following sets of elements could replace the generic "X" symbol with their own to produce a valid dot notation for the element(s)?
1. boron, aluminum and gallium
2. carbon, silicon and germanium
3. nitrogen, phosphorus and arsenic
4. oxygen, sulfur and selenium
Which of the following sets of elements could replace the generic "X" symbol with their own to produce a valid dot notation for the element(s)?
1. boron, aluminum and gallium
2. carbon, silicon and germanium
3. nitrogen, phosphorus and arsenic
4. oxygen, sulfur and selenium
Which of the following is the correct dot notation for the element carbon?
Which of the following is the correct dot notation for the element potassium, K?
Which of the following is the correct dot notation for the element sulfur?
Which of the following sets of elements could replace the generic "X" symbol with their own to produce a valid dot notation for the element(s)?
1. helium
2. neon
3. argon
4. radon
5. xenon
6. krypton
Identify the charge carried by a chloride ion.
1. 1-
2. 2-
3. 3-
4. 1+
5. 2+
6. 3+
Identify the charge carried by an oxide ion.
1. 1-
2. 2-
3. 3-
4. 1+
5. 2+
6. 3+
Identify the charge carried by a phosphide ion.
1. 1-
2. 2-
3. 3-
4. 1+
5. 2+
6. 3+
Identify the charge carried by a magnesium ion.
1. 1-
2. 2-
3. 3-
4. 1+
5. 2+
6. 3+
Identify the charge carried by an aluminum ion.
1. 1-
2. 2-
3. 3-
4. 1+
5. 2+
6. 3+
Identify the charge carried by a potassium ion.
1. 1-
2. 2-
3. 3-
4. 1+
5. 2+
6. 3+
What is the electron configuration of a sodium ion?
1. 1s²2s²2p⁶
2. 1s²2s²2p⁶3s¹
3. 1s²2s²2p⁶3s²
4. 1s²2s²2p⁶3s²3p⁶
What is the electron configuration of a sulfide ion?
1. 1s²2s²2p⁶
2. 1s²2s²2p⁶3s²3p⁴
3. 1s²2s²2p⁶3s²3p²
4. 1s²2s²2p⁶3s²3p⁶
What is the electron configuration of a calcium ion?
1. 1s²2s²2p⁶3s²3p⁴
2. 1s²2s²2p⁶3s²3p⁶4s²3d²
3. 1s²2s²2p⁶3s²3p⁶4s²
4. 1s²2s²2p⁶3s²3p⁶
When elements gain or lose electrons to form ions,
1. their nuclei become more stable
2. they have the electron configuration of a noble gas
3. they become noble gases
4. they become unstable
When forming ions, metals can be expected to _________ electrons while nonmetals can be expected to __________ gain electrons.
1. lose / gain
2. gain / lose
3. split / destroy
4. acquire / disperse
Ionic compounds are ordinarily found as
1. liquids
2. gases
3. plasma
4. crystals
Ionic compounds are held together by
1. electrostatic forces - opposites attract.
2. nuclear forces that overcome the repulsion of similar charges.
3. gravitational forces, since the ions are not the same size.
4. unknown forces - no one is certain what holds ionic compounds together.
Which of the following is the correct ionic compound formula for calcium sulfide?
1. CaS
2. Ca₂S
3. CaS₂
4. Ca₃S₂
Which of the following is the correct ionic compound formula for iron(III) oxide?
1. FeO
2. Fe₂O
3. Fe₃O₂
4. Fe₂O₃
Which of the following is the correct ionic compound formula for sodium iodide?
1. NaI
2. Na₂I
3. Na₃I₂
4. Na₃I
Which of the following is the correct ionic compound formula for copper(II) fluoride?
1. CuF₂
2. Cu₂F
3. Cu₂F₂
4. Cu₂F₃
Which of the following is the correct ionic compound formula for barium nitride?
1. BaN₂
2. Ba₂N
3. Ba₂N₃
4. Ba₃N₂
Pretend that a new alkaline earth metal, with an atomic number of 120 is produced. It would initially be given the symbol Ubn (Un-Bi-Nilium, or 1-2-0-ium). If you could react this new atom with the already synthesized halogen, Uus (Ununseptium, 117), what would be the formula of the ionic compound that they would form? (By the way, 117 is too unstable and would decay in a less than a millisecond. The same would likely be true of 120, so you could never actually test this out!)
1. UbnUus₂
2. Ubn₂Uus₃
3. Ubn₂Uus
4. UbnUus
What is the formula mass of calcium oxide, CaO, rounded to the ones place?
1. 56 grams
2. 72 grams
3. 48 grams
4. 28 grams
What is the formula mass of sodium nitride, Na₃N, rounded to the ones place?
1. 83 grams
2. 69 grams
3. 40 grams
4. 37 grams
What is the formula mass of chromium(III) fluoride, CrF₃, rounded to the ones place?
1. 109 grams
2. 71 grams
3. 51 grams
4. 81 grams
Which of the following pairs of elements would not react to form an IONIC compound?
1. iron and oxygen
2. sulfur and phosphorus
3. sodium and iodine
4. aluminum and bromine
Which of the following pairs of elements COULD react to form an ionic compound?
1. potassium and calcium
2. fluorine and copper
3. sulfur and oxygen
4. hydrogen and oxygen
When electrons are exchanged between metals and nonmetals, metals ________ electrons to form ____________.
Nonmetals ___________ electrons to form _____________.
1. lose / anions
  gain / cations
2. lose / cations
  gain / anions
3. gain / anions
  lose / cations
4. gain / cations
  lose / anions