Chem Unit 2: Exam #2 Prep
Choose the correct symbol of the sulfate ion. A. SO₄⁻ B. SO₃²⁻ C. S₄²⁻ D. SO₄²⁻ E. S₂⁻ F. SO₃⁻
D. SO₄²⁻
What is the charge on the monatomic ion of O?
2⁻
Choose the correct name for NO₃⁻ ion: A. nitrate ion B. nitrogen trioxide one minus ion C. nitrite ion D. nitride ion E. nitrogen trioxide ion
A. nitrate ion
Elemental nickel (Ni) has six stable isotopes. For each of the Ni isotopes which of these is constant? (Is the same for every isotope?) A. Mass number B. Number of electrons C. Number of neutrons D. Isotopic Mass
B. Number of electrons
The difference between the electronegativity of hydrogen and fluorine is approximately 1.8 (depending on the source). Which of the following describes the bonding in HF? A. Ionic B. Polar covalent C. Non-polar covalent D. Metallic
B. Polar covalent
Which of these lists has its elements in the correct order of INCREASING electronegativity? A. F < Br < I B. Rb < Ga < N C. O < Al < Ba D. B < Cs < Li E. P < Ge < K F. Cl < Si < S
B. Rb < Ga < N
Which of the following best describes what occurs with a difference in electronegatively? A. The MORE electronegative atom will hold onto the electrons within a bond more, making the atom more POSITIVE B. The MORE electronegative atom will hold onto the electrons within a bond more, making the atom more NEGATIVE C. The LESS electronegative atom will hold onto the electrons within a bond more, making the atom more NEGATIVE D. The LESS electronegative atom will hold onto the electrons within a bond more, making the atom more POSITIVE
B. The MORE electronegative atom will hold onto the electrons within a bond more, making the atom more NEGATIVE
Aluminum sulfate is ____ compound. Al₂(SO₄)₃ A. both an ionic and a covalent B. an ionic C. a covalent
B. an ionic
Magnesium phosphate is ____ compound. A. a covalent B. an ionic C. both an ionic and a covalent
B. an ionic
Which is a name that is necessarily incorrect? A. periodic acid B. dilithium monoxide C. sodium hydrogen carbonate D. hydrosulfuric acid
B. dilithium monoxide
Choose the correct name of this compound. FeF₃ A. monoiron trifluoride B. iron (III) fluoride C. iron fluorate D. iron fluoride E. iron fluorite
B. iron (III) fluoride
Arrange these compounds in order of decreasing attractions among ions. NaBr, Al₂O₃, MgO A. MgO > Al₂O₃ > NaBr B. Al₂O₃ > MgO > NaBr C. Al₂O₃ > NaBr > MgO D. MgO > NaBr > Al₂O₃ E. NaBr > Al₂O₃ > MgO F. NaBr > MgO > Al₂O₃3
C. Al₂O₃ > NaBr > MgO
CF₄ and CH₂F₂: Redraw both molecules to reflect the correct shape. After, draw the dipoles on the molecule. Do the dipoles cancel or reinforce each other? A. CH₂F₂: Reinforce CF₄: Reinforce B. CH₂F₂: Cancel CF₄: Cancel C. CH₂F₂: Reinforce CF₄: Cancel D. CH₂F₂: Cancel CF₄: Reinforce
C. CH₂F₂: Reinforce CF₄: Cancel
Choose the species that are isoelectronic with Li+. A. Ar, P³⁻, S²⁻, Cl- B. Ne, Mg²⁺, Al³⁺ C. He, H⁺, Be²⁺
C. He, H⁺, Be²⁺
The Al3+ ion is isoelectronic with ____ . A. Kr B. He C. Ne D. Xe E. Rn F. Ar
C. Ne
In magnesium phosphate, phosphate is ____ . A. an atom B. both an atom and a molecule C. a polyatomic ion D. an ion E. a molecule F. both an atom and an ion
C. a polyatomic ion
Choose the correct name of this compound. Cr(SO₄)₃ A. chromium sulfate B. chromium (II) sulfate C. chromium (VI) sulfate D. chromium (V) sulfate E. chromium (IV) sulfate F. chromium sulfite
C. chromium (VI) sulfate (Cr ⁶⁺ + SO₄ ²⁻)
A. NCl₃, PF₃, OCl₂
Choose the answer that contains all of the molecules from this list that are polar and none that are nonpolar. BF₃ NCl₃ CBr₄ PF₃ OCl₂ A. NCl₃, PF₃, OCl₂ B. BF₃, NCl₃, CBr₄ C. CBr₄, PF₃, OCl₂ D. NCl₃, CBr₄, OCl₂ E. BF₃, CBr₄, OCl₂ F. NCl₃, CBr₄, PF₃
C. sp²
Choose the correct hybridization of the atom indicated by arrow #3. A. sp B. sp³d C. sp² D. sp³d² E. sp³
E. sp³
Choose the correct hybridization of the atom indicated by arrow #4. A. sp B. sp³d C. sp² D. sp³d² E. sp³
The lattice energy of potassium chloride is -701 kJ/mole.Which is likely to be the lattice energy of cesium chloride? A. -834 kJ/mole B. -701 kJ/mole C. -2103 kJ/mole D. -657 kJ/mole
D. -657 kJ/mole
How many moles of oxygen (O) atoms are present in 34.18 g of sulfurous acid, H₂SO₃? A. 0.417 moles B. 2.398 moles C. 8.413 x 103 moles D. 1.250 moles E. 0.800 moles
D. 1.250 moles (H₂SO₃ molar mass = 82.07g/mol = 34.28g / 82.07g/mol = 0.4165 x 3 moles of O atoms present = 1.250 moles)
Choose the response that correctly identifies all of the ionic compounds in this list. Na₂SO₄ : H₂SO₄ : CH₃-CH₃ : N₂O₄ : CaCl₂ : Ca₃(PO₄)₂ A. CH₃-CH₃ N₂O₄ CaCl₂ B. Na₂SO₄ H₂SO₄ CaCl₂ C. N₂O₄ CaCl₂ Ca₃(PO₄)₂ D. Na₂SO₄ CaCl₂ Ca₃(PO₄)₂ E. Na₂SO₄ H₂SO₄ CH₃-CH₃ F. H₂SO₄ CH₃-CH₃ N₂O₄
D. Na₂SO₄ CaCl₂ Ca₃(PO₄)₂
In aluminum sulfate, aluminum is ____ . Al₂(SO₄)₃ A. both an atom and an ion without covalent bonds B. an atom C. an ion containing covalent bonds D. an ion E. a molecule F. both an atom and an ion
D. an ion
Choose the correct name of this compound. N₂O₅ A. nitro oxide B. dinitrogen monoxide C. nitric oxide D. dinitrogen pentoxide E. nitrogen oxide F. mononitrogen pentoxide
D. dinitrogen pentoxide
In 3.0 moles of Al2(SO4)3 there is/are ___ mole(s) of Al ions. A. 161.88 moles of Al B. 2.0 mole of Al C. 9.00 moles of Al D. 36.00 moles of Al E. 6.00 moles of Al F. 1.81 x 1024 moles of Al
E. 6.00 moles of Al
Choose the correct symbol of the carbonate ion. A. C₃²⁻ B. CO₂⁻ C. C₃⁻ D. CO₂²⁻ E. CO₃²⁻ F. CO³⁻
E. CO₃²⁻
Choose the correct symbol of the ammonium ion. A. NH₃²⁺ B. NH₄²⁺ C. N₃⁺ D. N₃²⁺ E. NH₄⁺ F. NH₃⁺
E. NH₄⁺
Choose the correct mass of 25.0 selenium (Se) atoms. A. 4.99 x 10⁻⁸ g B. 1.19 x 10²⁷ g C. 1,974 g D. 5.62 x 10⁻¹⁹ g E. 1.31 x 10⁻²¹ g F. 3.28 x 10⁻²¹ g
F. 3.28 x 10⁻²¹ g (molar mass x atoms / avo # ---> ( 78.971 x 25 / 6.022x10²³ = 3.28x10⁻²¹g)
True or false: The following compound contains polyatomic (molecular) ions: MnO₂
False
How many ions are present in one formula unit of magnesium phosphate? A. 1 B. 3.011 x 1024 C. 6.022 x 1023 D. 1.202 x 1024 E. 0 F. 2 G. 5
G. 5
What is the charge on the monatomic ion of Al?
3⁺
Choose the atom pair that will share their electrons most evenly forming the purest covalent bond. A. N and O B. K and Cl C. Na and Cl D. Ca and O E. As and F F. I and F
A. N and O
Choose the compound that contains a polyatomic ion. A. NaNO₃ B. CH₃OH C. CaBr₂ D. C₇H₁₄ E. NaCl F. AlN
A. NaNO₃ (also known as a molecular ion, is a charged chemical species (ion) composed of two or more atoms covalently bonded )
Based on your results in part 5, which would you say represents the trend in boiling point for these molecules? A. CH₂F₂ boils at a higher temperature than CF₄ B. CH₂F₂ boils at a lower temperature than CF₄ C. More information is necessary to determine boiling point trends D. CH₂F₂ boils at basically the same temperature as CF₄
A. CH₂F₂ boils at a higher temperature than CF₄
Which of the following describes the trend of electronegativity across the periodic table? A. Electronegativity decreases going down the periodic table and increases going to the right on the periodic table B. Electronegativity increases going down the periodic table and decreases going to the right on the periodic table C. Electronegativity decreases going down the periodic table and decreases going to the right on the periodic table D. Electronegativity increases going down the periodic table and increases going to the right on the periodic table
A. Electronegativity decreases going down the periodic table and increases going to the right on the periodic table
In magnesium phosphate, magnesium is ____ . A. an ion B. both an atom and a molecule C. an atom D. both an ion and a molecule E. a molecule F. both an atom and an ion
A. an ion
According to your answer in part one, which correctly identifies the change in energy based on bond breaking and forming for reactants and products? A Reactants form bonds, releasing energy Products break bonds, absorbing energy B Reactants form bonds, absorbing energy Products break bonds, releasing energy C Reactants break bonds, releasing energy Products form bonds, absorbing energy D. Reactants break bonds, absorbing energy Products form bonds, releasing energy
D. Reactants break bonds, absorbing energy Products form bonds, releasing energy
Choose the element that has the smallest atomic radius. A. Mg B. P C. Na D. Al E. Si F. S
F. S
HCO₃⁻ Lewis structure: Now, if necessary, add electrons as lone pairs from the outside in in order to complete octets. Only go until you have run out of electrons. If you added lone pairs, which elements did you put lone pairs onto? A. Hydrogen and Carbon B. Carbon Only C. Hydrogen Only D. Hydrogen and Oxygen E. Oxygen Only F. Oxygen and Carbon G. None of the elements H. Hydrogen, Oxygen, and Carbon
E. Oxygen Only
Determine the ionic charge of the positive ion in this ionic compound: SnBr₂
Sn = 2⁺
What is the molar mass of CaCl₂?
110.98g/mol
HCO₃⁻ Lewis structure: Add up all the valence electrons, including the charge. How many valence electrons?
24
How many oxygen (O) atoms are present in 27.7 g of Al₂O₃?
27.7 g x 1mol/101.96g x 6.02x10²³ atoms/mol = 1.64x10²³ x 3 (O) atoms = 4.91x10²³ atoms of O (in 27.7 g of Al₂O₃.)
Determine the ionic charge of the positive ion in the following ionic compound. Ni₃(PO₄)₂
2⁺
What is the charge on the common monatomic ion of Ca?
2⁺
Choose the total number of ions present in one formula unit of Al(NO₃)₃. A. 4 B. 2 C. 2.41 x 1024 D. 1 E. 13 F. 0
A. 4 ( 1- Al + 3 NO₃ ions)
Choose the correct formula of aluminum sulfate. A. Al₂(SO₄)₃ B. Al₃(SO₄)₂ C. Al₂S₃ D. AlS E. Al₂(SO₃)₃ F. Al(SO₄)₃
A. Al₂(SO₄)₃
Ethane burns in the presence of oxygen according to the following UNBALANCED reaction: ___C2H6 + ___O2 → ___H2O + ___CO2 Which of the following represents the correct ratio between ethane (C2H6) and CO2? A 2:1 B 1:2 C 1:3 D 3:1 E 1:1
B 1:2
We will now combine the two equations into a single formula to eliminate y and solve only for x. Which equation is appropriate for this calculation A 78.96*x + 80.90*(79.37-x) = 100 B 78.96*x +80.90*(1-x) = 79.37 C 78.96*x + 80.90*(79.37-x) = 1 D 78.96*x +80.90*(100-x) = 79.37
B 78.96*x +80.90*(1-x) = 79.37
E. B
What are the molecular geometries of the molecules XeF₄ and SF₄? A. E B. A C. D D. C E. B
C. 3 sigma bonds, 2 pi bonds
Which best describes the bonding in ethyne (HCCH)? A. 2 sigma bonds, 1 pi bond B. 2 sigma bonds, 1 pi bond, 1 delta bond C. 3 sigma bonds, 2 pi bonds D. 2 sigma bonds, 2 pi bonds
Determine the ionic charge of the positive ion in this ionic compound: MnO₂
Mn = 4⁺
Is the following compound covalent? CaBr₂
no
Is the following compound covalent? K₃N
no
Is the following compound covalent? Li₂O
no
Will the following combinations of elements form ionic compounds? N and Cl
no
Will the following combinations of elements form ionic compounds? N and O
no
How many moles of CaCl₂ are present in 65.5 grams of CaCl₂?
0.5902 mols (65.5/110.98)
How many moles of Cl⁻ ions are present in 65.5 grams of CaCl₂?
1.1804 mols (0.5902 mols x 2 Cl¹⁻ mole)
What is the charge on the monatomic ion of Ga?
3⁺
Draw the Lewis structure for PF3. How many electron groups are around the central atom?
4
Gold atoms have a radius of approximately 135 pm. If 4.63 x 1025 Au atoms were placed in a straight line with each Au atom touching its neighbor, how long, in miles, would the line extend? Note: 1 mile = 1.609 km
7.77 x 10¹² miles of Au atoms = (135 x 2 = diameter of circle = 270pm x 1 x10⁻¹⁵ km = 2.7 x 10⁻¹³ km diameter -----> x 1 mile/1.609 km = 1.678 x 10⁻¹³ miles per atom. ------> x 4.63 x 10²⁵ atoms of Au = 7.77 x 10¹² miles of Au atoms)
Elemental boron (B) has two stable isotopes 10B and 11B. A peculiar sample has isotopic abundances of 20% 10B and 80% 11B. (The isotopic mass of 10B is 10.0129 amu, and the isotopic mass of 11B is 11.0093 amu). What is the molar mass of this sample? A. 10 B. 10.8 C. 10.2 D. 11 E. 10.5
B. 10.8
Choose the ionic compound that has the largest melting point. (Hint: ionic bond strength determines melting points as well as solubility.) A. Al₂O₃ B. GaN C. NaCl D. CaS E. MgBr₂ F. Mg₃N₂
B. GaN
Choose the element which requires the GREATEST amount of energy to form a +1 ion. A. Na B. He C. K D. N E. Ne F. Cl
B. He
What is the correct chemical formula of magnesium phosphate? A. Mg₃PO₄ B. Mg₃(PO₄)₂ C. Mg₂PO₄ D. MgPO₄ E. Mg₂(PO₄)₃ F. Mg(PO₄)₃ G. Mg(PO₄)₂
B. Mg₃(PO₄)₂
Choose the element that has this electron configuration. [Kr] ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑ ↑ ⁻⁻⁻ ⁻⁻⁻ ⁻⁻⁻ ⁻⁻⁻ ⁻⁻⁻ ⁻⁻⁻ ⁻⁻⁻ 5s 4d A. Co B. Pd C. Ni D. Cd E. Ru F. Ag G. Rh H. Cu
B. Pd
Choose the element that has 5 valence electrons: A. I B. Sb C. Te D. Sr E. In F. Ar G. Ba
B. Sb
Sodium & oxygen make 3 different compounds together. 1)Sodium oxide: Na₂O 2) Sodium peroxide: Na₂O₂ (where peroxide is a diatomic oxygen ion w/ a -2 charge) 3) Sodium superoxide: NaO₂ (where superoxide is a diatomic oxygen ion w/ a -1 charge). Which compound will likely have the highest melting point, and why? A. Sodium superoxide, because the lattice energy will be lowest. B. Sodium oxide, because the lattice energy will be highest. C. None of them, because they are all essentially the same compound. D. Sodium peroxide, because the number of sodium and oxygen atoms is equal
B. Sodium oxide, because the lattice energy will be highest.
Which represents the molecular geometry of PF3? A. Trigonal Planar B. Tetrahedral C. Trigonal Bipyramidal D. Trigonal Pyramidal
B. Tetrahedral
Will the molecular geometry be different than the electron geometry? Why or why not? A. No, because the number of electron groups around the central atom does not change B. Yes, because the central atom has lone pairs C. No, because there are no lone pairs on the central atom D. Yes, because the outer atoms have lone pairs
B. Yes, because the central atom has lone pairs
Ca(NO₃)₂: This compound is composed of a(n) _____ and a(n) ____. A. positive molecule negative molecule B. positive ion negative molecular ion C. positive atom negative atom D. positive molecular ion negative ion E. positive atom neagtive ion
B. positive ion negative molecular ion
Using your ratios in parts 1 and 2, you will notice that there is an ODD number of oxygen atoms on the right side of the chemical reaction (1 O atom in H2O and 2 O atoms in CO2). The challenge is that there will always be an EVEN number of oxygens on the left (2 O atoms in O2). Which of the following could you do in order to account for this difference? A Remove two hydrogens from the formula of ethane B Divide everything in the reaction by two C Double everything in the reaction D Add an extra oxygen to the formula of water E Remove an oxygen from the fomula of O2
C Double everything in the reaction
What are the appropriate coefficients for balancing the following reaction. (The coefficients are in the same order as the substances.) Reaction: C6H6(l) + O2(g) --> CO2(g) + H2O(l) A. 1, 15, 12, 6 B. 1, 7, 6, 3 C. 2, 15, 12, 6 D. 1, 7, 12, 6
C. 2, 15, 12, 6
How many ions are present in one formula unit of aluminum sulfate? Al₂(SO₄)₃ A. 3.011 x 1024 B. 1 C. 5 D. 6.022 x 1023 E. 1.202 x 1024 F. 2 G. 0
C. 5
Which of the following correctly represents the change in energy when a bond is broken? A. Energy is released because because the kinetic energy increases B. Energy is released because entropy increases C. Energy is absorbed because bonds form to stabilize atoms D. Energy is released because the bond stores potential energy
C. Energy is absorbed because bonds form to stabilize atoms
A. AsCl₅
Choose the compound below that contains at least one polar covalent bond, but is nonpolar. A. AsCl₅ B. SCl₂ C. GeH₂Br₂ D. All of the choices are nonpolar and contain a polar covalent bond. E. CF₂Cl₂
C. sp²
Choose the correct hybridization of the atom indicated by arrow #1. A. sp B. sp³d C. sp² D. sp³d² E. sp³
D. sp³
Choose the correct hybridization of the atom indicated by arrow #2. A. sp B. sp³d C. sp² D. sp³ E. sp³d²
Which of the following correctly identifies the atom numbers and dipole direction? A. The student has not drawn a correct diagram: the atoms share the electrons equally B. 1: Fluorine 2: Hydrogen Dipole: Pointed toward 2 C. 1: Hydrogen 2: Fluorine Dipole: Pointed toward 1 D. 1: Hydrogen 2: Fluorine Dipole: Pointed toward 2 E. 1: Fluorine 2: Hydrogen Dipole: Pointed toward 2
D 1: Hydrogen 2: Fluorine Dipole: Pointed toward 2
Choose the correct answer to this problem based upon the correct number of significant figures. (451.300 x 165.178)(3.6 + 241.1)/37.994 = A. 4.8 x 10⁵ B. 4.8011 x 10⁵ C. 5 x 10⁵ D. 4.801 x 10⁵ E. 4.80 x 10⁵ F. 4.80105 x 10⁵
D. 4.801 x 10⁵ 1: (451.300*165.178)*(3.6+241.1)/37.994 2: (74544.831400*(3.6+241.1)/37.994 3: 74544.831400*(3.6+241.1)/37.994 4: 74544.8*(3.6+241.1)/37.994 5: 74544.8*(244.7/37.994 6: 74544.8*244.7/37.994 7: 74544.8*244.7/37.994 8: 18241112.56/37.994 9: 480105.0839606253618992 10: 480100 (Decimals: 0; Significant Figures: 4) Answer: 480100 OR 4.801 x 10⁵
A. Answer 1
Determine the electronic (electron pair) and the molecular geometry, as well as the polarity of PF5. 1. Trigonal bipyramidal/Trigonal bipyramidal/nonpolar 2. Octahedral/Octahedral/nonpolar 3. Trigonal bipyramidal/See-saw/polar 4. Octahedral/Trigonal bipyramidal/nonpolar 5. Tetrahedral/Tetrahedral /polar A. Answer 1 B. Answer 3 C. Answer 4 D. Answer 2 E. Answer 5
Which of the following describes the electronegativities of the elements in HF? A. Both atoms have the same electronegativity and will be neutrally charged B. Hydrogen is more electronegative than fluorine and will be more negatively charged C. Fluorine is more electronegative than hydrogen and will be more positively charged D. Hydrogen is more electronegative than fluorine and will be more positively charged E. Fluorine is more electronegative than hydrogen and will be more negatively charged
E Fluorine is more electronegative than hydrogen and will be more negatively charged
Choose the quantity that has the smallest number of O atoms. A. 96.0 g of O3 B. 64.0 g of O3 C. 96.0 g of O2 D. 64.0 g of O2 E. 48.0 g of O F. 96.0 g of O
E. 48.0 g of O
Elemental ___ commonly forms a(n) ___ with a ___ charge. A. N, anion, 2- B. Li, cation, 3+ C. Al, anion, 3- D. O, anion, 2+ E. Ca, cation, 2+ F. F, cation, 1-
E. Ca, cation, 2+
Choose the correct formula of calcium phosphate. A. Ca₂(PO₄)₃ B. Ca₃(PO₂)₂ C. Ca₂(PO₂)₃ D. CaPO₄ E. Ca₃(PO₄)₂ F. Ca₃P₂
E. Ca₃(PO₄)₂
Choose the correct chemical formula of the ionic compound formed when calcium (Ca) reacts with phosphorus (P). A. CaP₃ B. Ca₂P₃ C. CaP D. Ca₂P E. Ca₃P₂ F. Ca₃P G. CaP₂
E. Ca₃P₂
When aluminum becomes an ion, it has an electron configuration the same as which of the following? A. Argon B. Xenon C. Krypton D. None of the Above E. Neon F. Helium
E. Neon
C. tetrahedral, trigonal pyramidal
For NF₃ the electronic geometry is ___ and molecular shape is ____. A. tetrahedral, trigonal planar B. trigonal planar, tetrahedral C. tetrahedral, trigonal pyramidal D. tetrahedral, linear E. trigonal planar, trigonal planar
CF₄ and CH₂F₂.: Draw the Lewis structures for each of these molecules. After, draw dipoles for the molecules. Which of the following represents the correct direction of the dipoles for each molecule? A. From H to F B. From H to C C. From F to H D. From C to H E. From F to C F. From C to F G. Both from C to F and H to C
G. Both from C to F and H to C
What is the name of NH₄HCO₃ ?
ammonium bicarbonate Submit
Is the following element most likely to form a cation or an anion? F
anion
Is the following element most likely to form a cation or an anion? N
anion
Is the following element most likely to form a cation or an anion? Se
anion
Is the following element most likely to form a cation or an anion? Cs
cation
Is the following element most likely to form a cation or an anion? Rb
cation
s the following element most likely to form a cation or an anion? Ba
cation
F. Answer 5
Consider the molecule below. Determine the hybridization at each of the 3 labeled atoms. Atom 1/Atom 2/Atom 3 1. sp²/sp³/sp² 2. sp/sp²/sp² 3. sp³/sp²/sp 4. sp³/sp²/sp³ 5. sp³/sp²/sp² 6. sp³/sp³/sp³ A. Answer 3 B. Answer 4 C. Answer 2 D. Answer 1 E. Answer 6 F. Answer 5
Which angular momentum quantum number, l, corresponds to an orbital with a "dumbbell" shape geometry (two lobes opposite each other with a node at the nucleus). There are typically three such orbitals within any one principle quantum level. A. l = 3 B. l = -2 C. l = 0 D. l = 1 E. l = 2 F. l = -1
D. l = 1
What are the best systematic names for K₂CO₃ and N₂S₅? A. potassium carboxide, nitrogen (IV) sulfate B. dipotassium carbonate, nitrogen(II) sulfide C. potassium carbonate, nitrosulfide D. potassium carbonate, dinitrogen pentasulfide E. potassium(I) carbonate, dinitrogen pentasulfide F. potassium(I) carbonate, nitrogen(II) pentasulfide
D. potassium carbonate, dinitrogen pentasulfide
E. E
Determine the electronic geometry (electron pair geometry) and the molecular geometry, as well as the polarity of SeF₆ A. B B. C C. D D. A E. E
Choose the correct name of this compound - P₂S₅ A. phosphorus sulfite B. phosphorus (V) sulfide C. phosphorus sulfate D. phosphorus sulfide E. diphosphorus pentasulfide
E diphosphorus pentasulfide
HCO₃⁻ Lewis structure: Determine if there are any valid sites for additional resonance structures. If so, between what element could the additional bond be drawn? A. There is an additional bond, but no additional resonance structures. B. There are no additional bonds and no additional resonance structures. C. There is an additional structure by having an extra bond between O and a different O D. There is an additional structure by having an extra bond between H and a different O E. There is an additional structure by having an extra bond between C and a different O
E. There is an additional structure by having an extra bond between C and a different O
In aluminum sulfate, sulfate is ____ . Al₂(SO₄)₃ A. an ion without covalent bonds B. an atom C. both an atom and an ion D. a molecule E. an ion containing covalent bonds F. both an atom and a molecule
E. an ion containing covalent bonds
How many moles of platinum (Pt) are present in 192.5 g of platinum? A. 0.9867 moles B. 1.266 moles C. 1.233 moles D. 0.4934 moles E. 1.013 moles F. 0.5065 moles
A. 0.9867 moles( 192.5/195.084)
Choose the answer which has these ionic compounds correctly arranged in order of decreasing ionic bond strength. MgO AlP NaCl A. AlP > MgO > NaCl B. MgO > AlP> NaCl C. NaCl > MgO > AlP D. AlP > NaCl > MgO E. NaCl > AlP > MgO F. MgO > NaCl > AlP
A. AlP > MgO > NaCl
Choose the species that are isoelectronic with P3-. A. Ar, S²⁻, Cl⁻ B. As³⁻, Br⁻, Kr C. Ga³⁺, Ca²⁺, K⁺, Ar
A. Ar, S²⁻, Cl⁻
HCO₃⁻ Lewis structure: Now, if necessary, change lone pairs to additional bonds in order to complete octets for the remaining atoms. If you created any additional bonds, which of the following represents the pair of atoms between the bond? A. Between C and O B. There are no additional bonds C. Between C and H D. Between H and O
A. Between C and O
CH₂F₂ and CF₄: Which represents the polarity of the molecules? A. CH₂F₂: Polar CF₄: Non-Polar B. CH₂F₂: Non-Polar CF₄: Non-Polar C. CH₂F₂: Polar CF₄: Polar D. CH₂F₂: Non-Polar CF₄: Polar
A. CH₂F₂: Polar CF₄: Non-Polar
Choose the incorrect ground state electron configuration observed for the elements... A. Co electron configuration [Ar]4s¹3d⁸ B. Zn electron configuration [Ar]4s²3d¹⁰ C. Cr electron configuration [Ar]4s3¹d⁵ D. Br electron configuration [Ar]4s²3d¹⁰4p⁵ E. As electron configuration [Ar]4s²3d¹⁰4p³
A. Co electron configuration [Ar]4s¹3d⁸ (Should be Co:[Ar]4s¹3d⁷)
What is the formula for iron(II) phosphate? A. Fe₃(PO₄)₂ B. Fe₂PO₄ C. Fe₃PO₂ D. Fe₂P
A. Fe₃(PO₄)₂
Which of these acids is incorrectly named? A. HBrO Hydrobromic acid B. H₃PO₄ Phosphoric acid C. HNO₂ Nitrous acid D. H₂SO₄ Sulfuric acid E. HC₂H₃O₂ Acetic acid F. HCl Hydrochloric acid
A. HBrO (Correct: HypoBromous Acid)
Which of the following compounds are not ionic? (i.e if you dissolved them in water they would not split apart into cations and anions) Na₂SO₄ : P₄O₁₀ : CH₃-CH₃ : N₂O₄ : MgCl₂ : Ca₃(PO₄)₂ A. P₄O₁₀ CH₃-CH₃ N₂O₄ B. CH₃-CH₃ N₂O₄ MgCl₂ C. Na₂SO₄ N₂O₄ Ca₃(PO₄)₂ D. N₂O₄ MgCl₂ Ca₃(PO₄)₂ E. Na₂SO₄ P₄O₁₀ Ca₃(PO₄)₂ F. Na₂SO₄ MgCl₂ Ca₃(PO₄)₂
A. P₄O₁₀ CH₃-CH₃ N₂O₄
Based on your results in part 1, what would the electron geometry for PF3 be? A. Trigonal Bipyramidal B. Linear C. Octahedral D. Tetrahedral E. Trigonal Planar
A. Trigonal Bipyramidal
Ca(NO₃)₂: This compound is a(n) _____ compound. A. ionic B. both ionic and covalent C. covalent
A. ionic
Determine the ionic charge of the positive ion in this ionic compound: Co(NO₃)₂ (Write only the number without the charge)
Co= 2⁺
Choose the correct name for ClO₃⁻ ion: A. chloride ion B. perchlorate ion C. chlorine trioxide one minus ion D. chlorine trioxide ion E. chlorate ion F. chlorite ion
E. chlorate ion
Choose the correct name of this compound. Li₂S A. lithium sulfate B. lithium (I) sulfide C. lithium sulfite D. dilithium sulfide E. lithium sulfide
E. lithium sulfide
In the Lewis structure for acetonitrile there are ____ single bonds, ____ double bonds, ____ triple bonds and ___ lone pairs. A. 2-single; 1-double; 1-triple; 1-lone pair B. 3-single; 2-double; 0-triple; 2-lone pair C. 2-single; 2-double; 0-triple; 2-lone pair D. 3-single; 1-double; 1-triple; 1-lone pair E. 4-single; 2-double; 0-triple; 0-lone pair F. 4-single; 0-double; 1-triple; 1-lone pair
F. 4-single; 0-double; 1-triple; 1-lone pair
What is the correct chemical formula of aluminum sulfate? A. Al(SO₄)₂ B. Al₃SO₄ C. Al₃(SO₄)₂ D. AlSO₄ E. Al(SO₄)₃ F. Al₂(SO₄)₃ G. Al₂SO₄
F. Al₂(SO₄)₃
Choose the correct symbol of the phosphate ion. A. PO₃²⁻ B. P²⁻ C. PO₄²⁻ DP³⁻ E. PO₃³⁻ F. PO₄³⁻
F. PO₄³⁻
Choose the correct name for NH4+ ion: A. ammonite ion B. ammonia C. nitrogen trihydride plus one ion D. nitride ion E. nitrogen trihydride ion F. ammonium ion
F. ammonium ion
In acetonitrile the two C atoms are ___ hybridized and ___ hybridized. A. sp³ sp² B. sp³d sp³d C. sp³d sp D. sp³d² sp E. sp³ sp³d² F. sp³ sp
F. sp³ sp
True or false: The following compound contains polyatomic (molecular) ions: SnBr₂
False
E. trigonal planar, trigonal planar
For BF₃ the electronic geometry is ___ and molecular shape is ____. A. trigonal planar, tetrahedral B. tetrahedral, linear C. tetrahedral, trigonal pyramidal D. tetrahedral, trigonal planar E. trigonal planar, trigonal planar
Choose the correct formula of iron(III) oxide. A. Fe₂O B. FeO₂ C. FeO D. Fe₃O E. Fe₃O₂ F. FeO₃ G. Fe₂O₃
G. Fe₂O₃
A. N₂O > NO₂⁻ > NCl₃
Place the following in order of decreasing X-A-X bond angle, where A represents the central atom and X represents the outer atoms in each molecule. N₂O NCl₃ NO₂⁻ A. N₂O > NO₂⁻ > NCl₃ B. N₂O > NCl₃ > NO₂⁻ C. NO₂⁻ > N₂O > NCl₃ D. NCl₃ > NO₂⁻ >N₂O E. NCl₃ > N₂O > NO₂⁻
Is the following compound covalent? CF₄
yes
Is the following compound covalent? HI
yes
Is the following compound covalent? OBr₂
yes
Will the following combinations of elements form ionic compounds? Ca and I
yes
Will the following combinations of elements form ionic compounds? K and P
yes
Will the following combinations of elements form ionic compounds? Rb and S
yes
A Grain of sand has a mass of about 3.50x10⁻⁷ g. What is the mass of 1 mole of the sand grains?
3.50x10⁻⁷ g x 6.022 x 10²³ atoms /1 mole = 2.11 x 10¹⁷ g/mole
Analytical balances are sometimes used in upper level chemistry lab courses. An especially good analytical balance can detect as little as 0.0001 mg of a substance. How many glucose molecules, C6H12O6, are present in 0.00068 mg of glucose?
0.00000068g x 1mole/180.1559g x 6.02x10²³/1 mole = 2.27 x 10¹⁵
How many moles of Ca²⁺ ions are present in 65.5 grams of CaCl₂?
0.5902 mols (0.5902 mols x 1 Ca²⁺ mole)
What is the charge on the monatomic ion of Li?
1⁺
What is the charge on the monatomic ion of Br?
1⁻
What is the charge on the monatomic ion of Cl?
1⁻
What is the charge on the monatomic ion of Na?
1⁻
What is the charge on the common monatomic ion of Sr?
2⁺
What is the charge on the monatomic ion of S?
2⁻
Ca(NO₃)₂: In one formula unit of this compound there are ____ ions.
3
Bromine only has two naturally occuring isotopes: Bromine-79 and Bromine-81. You obtain a strange sample of bromine that has a mass of 79.37 amu. Additionally, you know that the mass bromine-79 is 78.96 amu, and bromine-81 weights 80.90 amu. Based on the atomic mass of this sample, which accurately represents the most abundant isotope of bromine in this sample. A Bromine-81, because the atomic mass of the sample is closer to 81 B Bromine-79, because the atomic mass of the sample is closer to 79 C Nearly identical abundances because the mass of the sample is about halfway between the two masses D Cannot be determined given this data
B Bromine-79, because the atomic mass of the sample is closer to 79
We will create two equations and two unknowns to determine the relative abundance of each isotope. The variable 'x' will represent the abundance of bromine-79, while the variable 'y' will represent the abundance of bromine-81. Which set of equations will best help us determine the values of x and y? A x + y = 79.37 78.96*x + 80.90*y = 1 B x + y = 1 78.96*x +80.90*y = 79.37 C x + y = 100 78.96*x +80.90*y = 79.37 D x + y = 79.37 78.96*x + 80.90*y = 100
B x + y = 1 78.96*x +80.90*y = 79.37
CF₄ and CH₂F₂.: Which represents the shape of these molecules? A. Square Planar B. Tetrahedral C. Linear D. Trigonal Planar E. Trigonal Pyramidal
B. Tetrahedral
In the unbalanced reaction in part 1, what must be the ratio between ethane (C2H6) consumed and water produced? A 1:1 B 3:1 C 1:3 D 1:2 E 2:1
C 1:3
A. sp
Choose the correct hybridization of the atom indicated by arrow #5. A. sp B. sp³d C. sp² D. sp³d² E. sp³
F. PCl₃
Choose the molecule that has a tetrahedral electronic geometry, trigonal pyramidal molecular geometry, and is polar. A. BeCl₂ B. BF₃ C. CCl₄ D. OF₂ E. SiH₂F₂ F. PCl₃
Lewis structures for the following molecules, following the pattern above: BeF2, HCN, BH3, SF6 Which of the above structures break the octet rule? A. HCN, BH3, and SF6 B. BeF2 and HCN C. BeF2 and BH3 D. HCN and SF6 E. All four structures F. BeF2 and SF6 G. BeF2, HCN, and BH3 H. HCN and BH3 I. BeF2, HCN, and SF6 J. BeF2, BH3, and SF6 K. None of the structures
J. BeF2, BH3, and SF6
Determine the ionic charge of the positive ion in this ionic compound: (NH₄)2CO₃
NH₄ = 1⁺
Determine the ionic charge of the positive ion in this ionic compound: Ni₃(PO₄)₂ (Write only the number without the charge)
Ni = 2⁺
E. sp³d
Which of the following correctly identifies the hybridization of ClF₃? A. sp³d² B. sp² C. sp³ D. sp E. sp³d
True or false: The following compound contains polyatomic (molecular) ions: (NH₄)₂CO₃
True (NH₄ - Ammonium)
True or false: The following compound contains polyatomic (molecular) ions: Co(NO₃)₂
True (NO₃⁻ - nitrate)
True or false: The following compound contains polyatomic (molecular) ions: Ni₃(PO₄)₂
True (PO₄³⁺ - phosphate)
E. -81. kJ
Using the tabulated bond energies provided, estimate the amount of heat transfer ( ΔHrxn/ ΔErxn) when the following reaction is performed. Assume the balanced equation accurately describes the number of moles of reactants and products involved. N2 + 3H2 → 2NH3 Nitrogen-Nitrogen Triple Bond: 945 kJ/mole Hydrogen-Hydrogen Single Bond: 436 kJ/mole Nitrogen-Hydrogen Single Bond: 389 kJ/mole A. -1865 kJ B. -863 kJ C. +81. kJ D. +993 kJ E. -81. kJ F. +1087 kJ
D. XeF₄: Square Planar, SF₄: See-Saw
What are the molecular geometries of the molecules XeF₄: and SF₄:? A. XeF₄: Tetrahedral, SF₄: Tetrahedral B. XeF₄: Tetrahedral, SF₄: Square Planar C. XeF₄: See-Saw, SF₄: Tetrahedral D. XeF₄: Square Planar, SF₄: See-Saw E. XeF₄: Square Planar, SF₄: Square Planar
B. sp₂
What is the hybridization of the central oxygen in the ozone molecule? (O₃) A. sp₃ B. sp₂ C. not hybridized D. sp
D. Octahedral 90°
Xenon tetrafluoride (XeF4) has a(n) ______ electronic (electron pair) geometry and bond angles of ____. A. Octahedral 120° B. Square planar 180° C. See-saw 109.5° D. Octahedral 90° E. Tetrahedral 109.5° F. Octahedral 109.5° G. See-saw 120° H. Square planar 120° I. Tetrahedral 90°
