Study for midterm - questions and answers from the worksheets
How many electrons does a fluorine atom gain to form a fluoride anion?
1
How many electrons does a fluoride anion contain?
10
How many electrons does a magnesium cation contain?
10
How many electrons does a sodium cation contain?
10
How many electrons does a neutral magnesium atom contain?
12
How many electrons does a magnesium atom lose to form a magnesium cation?
2
Which group on the periodic table contains fluorine (F)?
7
How many electrons does a neutral fluorine atom contain?
9
Which group on the periodic table contains Magnesium (Mg)?
Group 2
Would you expect carbon monoxide and carbon dioxide to be polar or non polar molecules?
I would expect them to be non polar molecules
What is the relationship between the group number of the representative elements and the number of valence electrons.
The number of valence electrons in an atom of a representative element is the same as the group number of the element.
How many valence electrons does each of the following atoms have? a. gallium b. fluorine c. selenium
a. # of valence electrons = 3 b. # of valence electrons = 7 c. # of valence electrons = 6
Write the formulas for compounds formed from these pairs of ions. a.NH4^+, SO4^2- b. K+, NO3^- c. barium ion and hydroxide ion d. lithium ion and carbonate ion
a. (NH4)2SO4 b. KNO3 c. Ba(OH)2 d. Li2CO3
For each element below, state (i) the number of valence electrons in the atom, (ii) the electron dot structure, and (iii) the chemical symbol(s) for the most stable ion. a. Ba b. I c. K
a. (i) # of valence electrons = 2, (ii) Ba - 1 on the right and 1 on the top (could honsestly be anywhere), (iii) - Ba2+ b. (i) - # of valence electrons = 7, (ii) I - two dots on all sides except for the bottom which only has one, (iii) - I- c. (i) - # of valence electrons = 1, (ii) K - 1 on the right, (iii) K+
Find the Molar Mass of the following compounds: a. LiI b. AgF c. K3PO4 d. C6H12O6 e. PbCO4 f. Mg(OH)2
a. 134 g b. 127 g c. 212 g d. 180 g e. 283 g f. 58 g
How many electrons does each of the following ions contain? a. S^2- b. Ca^2+ c. K^+ d. Cl^-
a. 18 b. 18 c. 18 d. 18
Write the electron configuration for each of the following atoms or ions. a. Ca b. chlorine atom c. Na+ d. phosphide ion e. O2-
a. 1s2, 2s2, 2p6, 3s2, 3p6, 4s2 b. 1s2, 2s2, 2p6, 3s2, 3p5 c. 1s2, 2s2, 2p6 (this is lacking the 3s level because an electron was taken away) d. 1s2, 2s2, 2p6, 3s2, 3p6 ( this is 6 instead of 3 because it had achieved a stable octet) e. 1s2, 2s2, 2p6 (again, this electron configuration is 2p6 instead of 2p4 because it gained 2 electrons)
What is the charge on the ion typically formed by each element? a. oxygen b. iodine c. sodium d. aluminum e. nickel, 2 electrons lost f. magnesium
a. 2- b. 1- c. 1+ d. 3+ e. 2+ f. 2+
Write the formulas for the compounds formed from these pairs of ions. a. Ba2+, Cl- b. Ag+, I- c. Ca2+, S2- d. K+, Br- e. Al3+, O2- f. Fe2+. O2-
a. BaCl2 b. AgI c. CaS d. KBr e. Al2O3 f. FeO
Write the formula (including the charge) for each ion. Use Table 9.3 if necessary. a. carbonate ion b. nitrite ion c. sulfate ion d. hydroxide ion e. chromate ion f. ammonium ion
a. CO3^2- b. NO2^-2 c. SO4^2- d. OH- e. CrO4^2- f. NH4^+
Give the name and symbol of the ion formed when a. a chlorine atom gains one electron b. a potassium atom loses one electron c. an oxygen atom gains two electrons d. a barium atom loses two electrons
a. Cl- b. K+ c. O2- d. Ba2+
Name the following binary ionic compounds. a. MnO2 b. Li3N c. CaCl2 d. SrBr2 e. NiCl2 f. K2S g. CuCl2 h. SnCl4
a. Maganese (II) Oxide b. Lithium Nitride c. Calcium Chloride d. Strontium Bromide e. Nickel (II) Chloride f. Potassium Sulfide g. Copper (II) Chloride h. Tin (IV) Chloride
Write the formulas for these binary ionic compounds. a. magnesium oxide b. tin(II) fluoride c. potassium iodide d. aluminum chloride e. sodium sulfide f. ferric bromide
a. MgO b. SnF2 c. KI d. AlCl3 e. Na2S f. FeBr3
Write the formulas for the following binary molecular compounds. a. nitrogen tribromide b. dichlorine monoxide c. sulfur dioxide d. dinitrogen tetrafluoride
a. NBr3 b. Cl2O c. SO2 d. N2F4
Write the formulas for the following ionic compounds. a. sodium phosphate b. magnesium sulfate c. sodium hydroxide d. potassium cyanide e. ammonium chloride f. potassium dichromate
a. Na3P b. MgS c. NaOH d. KCN e. NH4Cl f. K(CrO4^2-)2
Use the electron dot structures to predict the formula of the ionic compounds formed when the following elements combine. a. sodium and bromine b. sodium and sulfur c. calcium and iodine d. aluminum and oxygen e. barium and chlorine
a. NaBr b. Na2S c. CaI6 d. Al2O3 e. BaCl6
Name the following molecular compounds. a. PCl5 b. CCl4 c. NO2 d. N2F2 e. P4O6 f. XeF2 g. SiO2 h. Cl2O7
a. Phosphorus Pentachloride b. Carbon Tetrachloride c. Nitrogen Dioxide d. dinitrogen difluoride e. tetraphosphorus hexaoxide f. Xenon Difluoride g. silicon dioxide h. dichloride heptaoxide
Name these compounds. a. NaBr b. SiO2 c. BBr3 d. LiI e. GaAs f. GaCl3 g. B2H4 h.K2O i. SCl2 j. CO
a. Sodium Bromide b. Silicon dioxide c. Boron tribromide d. Lithium Iodide e. Gallium Arsenide f. Gallium Chloride g. Diboron tetrahydride h. Potassium oxide i. Sulfur dichloride j. Carbon monoxide
Name the following compounds. a. NaCN b. FeCl3 c. Na2SO4 d. K2CO3 e. Cu(OH)2 f. LiNO3
a. Sodium Cyanide b. Iron (III) Chloride c. Sodium Sulfate d. Potassium Carbonate e. Copper (II) Hydroxide f. Lithium Nitrate
Name and give the charge of the metal cation in each of the following ionic compounds. a. Na3PO4 b. NiCl2 c. CaS d. K2S e. FeCl3 f. CuI
a. Sodium, 2+ b. Nickel, 2+ c. Calcium, 2+ d. Potassium, 1+ e. Iron, +3 f. Copper, +1
Classify each of the following as an atom or a molecule. a. Be b. CO2 c. N2 d. H2O e. Ne
a. atom b. molecule c. molecule d. molecule e. atom
Classify each of the following as a cation or an anion. a. Na+ b. Cu2+ c. I- d. O2- e. Ca2+ f. Cs+
a. cation b. cation c. anion d. anion e. cation f. cation
Label each as covalent (nonmetal + nonmetal) or ionic (metal + nonmetal): a. NO2 b. NaCl c. SO2 d. PO4^3- e. MgBr2 f. CaO g. H2O h. K2O i. O2 j. CuCl2 k. NO2 l. TiO2 m. HF n. Rb2S o. Fe2O3 p. C6H12O22
a. covalent b. ionic c. covalent d. covalent e. ionic f. ionic g. covalent h. ionic i. covalent j. ionic k. covalent l. ionic m. covalent n. ionic o. ionic p. covalent
Name the following ions. Identify each as a cation or an anion. a. CN- b. HCO3^- c. PO4^-3 d. Cl- e. Ca^2+ f. SO3^2-
a. cyanide anion b. hydrogen carbonate anion c. phosphate anion d. chloride anion e. calcium cation f. sulfite anion
What type of bond - nonpolar covalent, polar covalent, or ionic - will form between each pair of atoms? a. Na and O b. O and O c. P and O
a. ionic b. polar covalent c. nonpolar covalent
How many electrons will each element gain or lose in forming an ion? State whether the resulting ion is a cation or an anion. a. strontium b. aluminum c. tellurium d. rubidium e. bromine f. phosphorus
a. lose 2, cation b. lose 3, cation c. gain 2, anion d. lose 1, cation e. gain 1, anion f. gain 3, anion
How many electrons does the neutral atom gain or lose when each ion forms? a. Cr3+ b. P3- c. Li+ d. Ca2+ e. Cl- f. O2-
a. lose 3 b. gain 3 c. lose 1 d. lose 2 e. gain 1 f. gain 2
How many electrons are lost or gained in forming each of the following ions? a. Mg2+ b. Br- c. Ag+ d. Fe3+
a. lost 2 b. gained 1 c. lost 1 d. lost 3
Which of the following are diatomic molecules? a. CO2 b. N2 c. O2 d. H2O e. CO
a. not diatomic b. diatomic c. diatomic d. not diatomic e. diatomic
Name each ion. Identify each as a cation or an anion. a. Sn2+ b. Co3+ c. Br- d. K+ e. H- f. Mn2+
a. tin (II) or stannous cation b. cobalt (III) or cobalitic cation c. Bromide anion d. Potassium cation e. Hydride anion f. Manganese (II) or manganous cation
Which of these combinations of elements are most likely to react to form ionic compounds? a. sodium and magnesium b. barium and sulfur c. potassium and iodine d. oxygen and argon
c. potassium and iodine b. barium and sulfur
What is a metallic bond?
the force of attraction that holds metals together; it consists of the attraction of free-floating valence electrons for positively charged metal ions
What is the meaning of the coordination number?
the number of ions of opposite charge that surround each ion in a crystal
