Chemistry

How many moles of NaNO3 are present in a 44.0 g sample? 0.518 0.44 1.14 44

0.518

The Lewis symbol for sodium will have how many dots? Report your answer as an integer (whole number) without any decimal places. Do not include units in your response.

1

Given the fictitious chemical equation below: 1 tablespoon of dry tea+2 cups of water⟶ 2 cups of tea What is the appropriate stoichiometric factor relating the two "reactants"? 1 cup of H2O/1 cup of tea 1 tbsp dry tea/2 cups H2O 1 tbsp tea/2 cups of tea 1 tbsp dry tea/2 cups of tea

1 tbsp dry tea/2 cups H2O

Fill in the blank coefficients in order to balance the following chemical equation. Your answers should be whole numbers; use 1 if there is no coefficient. ___H2o2 ____SO2 ____H2SO4

1,1,1

If a sample of CO2 contains 48 grams oxygen, how many moles of CO2 are there? 0.5 1 1.5 2

1.5

What will be the mass of one mole of carbon atoms? 12 g 12 amu 6.022×1023 g 6.022×1023 amu

12 g

Identify the balanced chemical equation. 2 O2+4 Fe→2 Fe2O3 C7H16+10 O2→7 CO2+8 H2O FeBr3+H2SO4→Fe2(SO4)3+HBr 2 Fe+3 Cl2→2 FeCl3

2 Fe+3 Cl2→2 FeCl3

In the equation 5Z→2A+3B, how many molecules of Z must react to give 15 molecules of B?

25 Molecules of Z

What is the coefficient for O2 in the balanced version of the following chemical equation: C2H4+O2→CO2+H2O

3

What is the coefficient for Fe(s) in the balanced version of the following chemical equation: ___?Fe(s)+___O2(g)→___Fe2O3(s)

4

Using the chemical equation provided, identify which of the following are the coefficients of the reactants. 4Fe+3O2⟶2Fe2O3 7 4 3 2

4 3

What is the mass in grams of 3.7 moles CH4? 16 g 59 g 67 g 89 g

59 g

According to the following reaction, how many moles of Cl2 must react in order to produce 4 moles AsCl3?2As+3Cl2→2AsCl3 8 6 4 2

6

How many moles of hydrogen atoms are in 8 g H2? 2 4 8 16

8

How many grams of oxygen are there in 2.5 moles of oxygen (O2) molecules? 16 g 40. g 80. g 120 g

80. g

What is the mass in grams of 5.50 moles NH3? 93.5 550 17 117

93.5

Barium phosphate is formed from the Ba2+ cation and the PO3−4 anion. What is the correct formula for this compound?

Ba3(PO4)2

Carbon tetrabromide has the formula __________. CBr2 CBr3 CBr4 CBr5

CBr4

Which of the following would have the higher boiling point? CH3CN C3H8 They have the same boiling point. There is not enough information to determine this.

CH3CN

Cesium sulfite is formed from the Cs+ cation and the SO2−3 anion. What is the correct formula for this compound?

Cs2SO3

Copper (II) iodide is formed from the Cu2+ cation and the I− anion. What is the correct formula for this compound?

CuI2

Hydrogen bonding is responsible for:

DNA base pairing

Identify the missing product in the following acid-base reaction. Include the coefficient only if it is larger than 1 in the balanced equation. Fe(OH)2 + 2HF -> _______ 2H2O

FeF2

Use the figure provided to determine which of the following has bonds with the greatest bond-polarity? HCl NO2 NH3 H2O

H2O

Identify the compound(s) with polar covalent bonds. Cl2 H2O NO2 AlBr3

H2O NO2

Identify the compound(s) containing polar covalent bonds. F2 HBr N2 CO2

HBr CO2

Which of the following dissolves in water to yield hydronium ions? Select all that apply. NaCl HBr HNO3 HI

HBr HNO3 HI

Which of the following is a molecular compound? HF NaF CaCl2 MgO

HF

Which of the following will have the highest boiling point? HCl HF HBr they have the same boiling point

HF

Use the figure provided to determine which of the following is the least polar. CO HCl ICl NaCl

ICl

Identify the missing product in the following acid-base reaction. Include the coefficient only if it is larger than 1 in the balanced equation. H2CO3 + 2 LiOH -> ____________ 2H2O

Li2CO3

Na2O consists of __________. Na+ and O− ions Na2+ and O− ions Na2+ and O2− ions Na+ and O2− ions

Na+ and O2− ions

Identify the molecules(s) containing non-polar covalent bonds. O2 SF6 H2 NO2

O2 H2

Which of the following is the correct molecular formula for the binary compound: tetraphosphorus decaoxide? P10O4 PO P4O10 P2O5

P4O10

Which of the following has dipole-dipole attractions? CO2 F2 FeCl2 PCl3

PCl3

What is the molecular formula for phosphorus pentachloride? PCl5 PCl P5Cl P5Cl5

PCl5

Sulfur hexafluoride has the formula SF5. SF6. SF7. SF8.

SF6.

All of the following compounds feature ionic bonds except __________. Li2O SO2 Ca3P2 FeO

SO2

Which of the following is NOT a molecular compound? SnSe2 NH3 PCl5 N2O4

SnSe2

In general, covalent bonding can occur between which of the following? An ion and a neutral atom Two ions of opposite charge Two neutral atoms Any combination above

Two neutral atoms

------ = Single Bond, Shared pair (2) electrons .. = Lone Pair, electrons not used in bonding

Use the image below to answer the question that follows. Which of the following is an appropriate key for the image above?

Hydrogen bonds are exceptionally strong because: they involve exceptionally strong dipoles hydrogen atoms are very small fluorine, oxygen, and nitrogen atoms are relatively small all of the above

all of the above

Name the following molecule: CCl4. monocarbon tetrachloride carbon chloride carbon tetrachloride carbon dichloride

carbon tetrachloride

A mole is defined as the number of atoms in an exact mass of which isotope? nitrogen-14 hydrogen-1 oxygen-18 carbon-12

carbon-12

In a chemical equation, the number of molecules (or formula units) of a particular substance that are participating in the chemical reaction is indicated by a: coefficient forward arrow plus sign subscript

coefficient

Using the strict IUPAC naming convention for binary molecular compounds, the name for water (H2O) would be __________. hydrogen oxide dihydrogen oxide hydrogen monoxide dihydrogen monoxide

dihydrogen monoxide

Intermolecular forces are all some kind of: gravitational attraction nuclear repulsion electrostatic attraction none of the above

electrostatic attraction

Nitrogen monoxide, NO, is formed in internal combustion engines by the reaction below. N2(g)+O2(g)+energy(heat)⟶2NO(g) Is the production of NO endothermic or exothermic? endothermic exothermic neither endothermic nor exothermic both endothermic and exothermic

endothermic

This is the reaction that happens inside of a cold pack found in emergency kits: NH4NO3(s)⟶NH4NO3(aq) Is the reaction endothermic or exothermic? endothermic exothermic neither endothermic nor exothermic both endothermic and exothermic

endothermic

Is the following process endothermic or exothermic? H2O(g)⟶H2O(l) endothermic exothermic neither endothermic nor exothermic both endothermic and exothermic

exothermic

Is the following process endothermic or exothermic? H2O(l)⟶H2O(s) endothermic exothermic neither endothermic nor exothermic both endothermic and exothermic

exothermic

This is the reaction that happens inside of a hot pack found in emergency kits: CaCl2(s)⟶CaCl2(aq) Is the reaction endothermic or exothermic? endothermic exothermic neither endothermic nor exothermic both endothermic and exothermic

exothermic

Which of the following is the correct name for F−? fluorion fluorine ion fluorine fluoride

fluoride

Polar molecules have attractive dipole-dipole interactions when the dipoles are arranged in which of the following geometries?

head-to-tail: →→ side-to-side, antiparallel: ↑↓

Intermolecular forces are primarily responsible for: holding together the atoms in a molecule holding together molecules in a material both a and b none of the above

holding together molecules in a material

The kinetic energies of molecules are responsible for: holding molecules close together increasing the distance between particles changing the magnitude of intermolecular attractions none of the above

increasing the distance between particles

IF7 is called iodine hexafluoride. monoiodine hexafluoride. iodine heptafluoride. monoiodine heptafluoride.

iodine heptafluoride.

Which of the following correctly pairs the ion name with the ion symbol? iodine, I− sulfite, S2− lithium cation, Li+ nitride, N−

lithium cation, Li+

MgCl2 is called __________. magnesium dichloride magnesium chlorate monomagnesium chlorate magnesium chloride

magnesium chloride

What results when two or more atoms share electrons equally? molecular compounds ionic compounds polar compounds polyatomic compounds

molecular compounds

When naming binary covalent compounds, the element listed first will be the one that is more metallic. less metallic. heavier. lighter.

more metallic.

Which of the following is the correct name for N3−? nitrous ion nitrogen ion nitride nitrine

nitride

The number of atoms in one mole of oxygen is equal to the number of atoms in ______ of hydrogen. a quarter of a mole half a mole one mole two moles

one mole

In a polar covalent bond, the more electronegative atom will bear a: formal negative charge formal positive charge partial negative charge partial positive charge

partial negative charge

Intermolecular forces determine the _____ of a substance. mass volume phase temperature

phase

What is the name of the compound PCl5? phosphorus hexachloride phosphorus pentachloride phosphorus tetrachloride phosphorus trichloride

phosphorus pentachloride

What types of particles can participate in dipole-dipole interactions? polar molecules nonpolar molecules ions any particles

polar molecules

A base is something that: gives up an H+ ion when dissolved in water. produces an OH− ion when dissolved in water. gains an OH− ion when dissolved in water. none of the above

produces an OH− ion when dissolved in water.

Converting from moles of one compound into moles of another compound in a chemical equation will require the: molar masses molecular masses stoichiometric factor molecular geometries

stoichiometric factor

In a chemical equation, the number of atoms of a particular element that are present in a substance is indicated by a: coefficient forward arrow plus sign subscript

subscript

If we compare a mole of carbon atoms to a mole of oxygen atoms, which sample will contain more mass? the carbon sample the oxygen sample they will contain the same mass impossible to tell

the oxygen sample

In an endothermic reaction, do the reactants or the products have more heat energy? the reactants the products

the products

Coefficients in a chemical formula provide: the relative numbers of products and reactants the absolute number of products and reactants the number of reactants only the number of products only

the relative numbers of products and reactants

Hydrogen bonding is responsible for: the unexpectedly high boiling points for hydrides in period two the increasing boiling points for hydrides going down a group the low boiling points of nonpolar molecules none of the above

the unexpectedly high boiling points for hydrides in period two

Noble gases do not receive electronegativity values because: they are too difficult to measure they are gases they do not form covalent bonds none of the above

they do not form covalent bonds

If we compare a mole of carbon atoms to a mole of oxygen atoms, which sample will contain more atoms? the carbon sample the oxygen sample they will contain the same number of atoms impossible to tell

they will contain the same number of atoms

Use the image below to answer the question that follows. .Ca. The dots in the image above represent:

valence electrons