Chemistry Final Exam

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The formula that a compound ammonium sulfide is _______________.

(NH4)2S

The formula for the compound ammonium sulfate is.

(NH4)2SO4

What is the charge on the cation in CuSO4?

+2

What is the ionic charge on the titanium ion in the ionic compound titanium oxide, TiO2?

+4

What is the ionic charge on the zirconium ion in the ionic compound zirconium oxide, ZrO2?

+4

What is the charge on the anion in CuSO4?

-2

To prevent tooth decay, many communities treat their water supply with a fluoride compound such as CaF2. How many kilograms of CaF2 would be necessary to treat 287 kL of water to a concentration of 1.00 mg/L of CaF2?

.287 kg

Determine the subscript for dichromate in the chemical formula for ammonium dichromate.

0

How many unshared pairs does an atom of boron contain in its Lewis structure?

0

___Ba + ___H2O --> ___Ba(OH)2 + ___H2

0, 2, 0, 0

___(NH4)2CO3 + ___NaOH --> ___Na2CO3 + ___NH3 + ___H2O

0, 2, 0, 2, 2

___Cd(NO3)2 + ___NH2Cl -->

0, 2, CdCl2 + 2NH4NO3

___CH4 + ____________ --> H2O + _________________

0, 2O2 --> 2, CO2

___C2H5OH + ___O2 --> ___CO2 + ___H2O

0, 3, 2, 3

___Fe2(SO4)3 + ___Ba(OH)2 -->

0, 3, 2Fe(OH)3 + 3BaSO4

___C3H6 + ___O2 ---> ___CO + ___H2O

0, 3, 3, 3

What is the molarity of a solution that contains 0.202 mol KCl in 7.98 L solution?

0.0253 M

How many moles of HCl are present in 0.70 L of a 0.33 M HCl solution?

0.23 mol

What is the number of kilograms of solvent in a 0.70 molol solution containing 5.0 grams of solute? (molar mass of solute= 30 g)

0.24 kg

What is the molarity of a solution that contains 125 g NaCl in 4.00 L solution?

0.535 M

How many iron(II) ions combine with oxygen to form iron(II) oxide?

1

What is the expression of molality?

10 mol of solute/ 1 kg of solvent

Determine the subscript for ammonium in the chemical formula for ammonium dichromate.

2

How many electrons are shared in a single covalent bond?

2

How many iron (III) ions combine with oxygen to form iron (III) oxide?

2

___Al + ___Cl2 -->

2, 3, 2AlCl3

___ Na3PO4 + ___ZnSO4 --> ___Na2SO4 + ___Zn3(PO4)2

2, 3, 3, 0

___Au2O3 --> ___Au + ___O2

2, 4, 3

___C3H8 + ___O2 -> ___CO + ___H2O

2, 7, 6, 8

The density of acetylene at STP is 1.17 g/L. The empirical formula of acetylene is CH. Determine the molar masses of acetylene and its molecular formula.

26.2g : C2H2

How many electrons does phosphorous need to gain in order to obtain a noble-gas electron configuration?

3

How many unshared pairs of electrons are in a molecule of hydroiodic acid?

3

What is the total number of covalent bonds normally associated with a single nitrogen atom in a compound?

3

___Mg + ___H3PO4 --> ___Mg3(PO4)2 + ___H20

3, 2, 0, 3

An NaOH solution contains 1.90 mol of NaOH, and its concentration is 0.555 M. What is its volume?

3.42 L

When a mixture of sulfur and metallic silver is heated, silver sulfide is produced. What mass of silver sulfide is produced from a mixture of 3.0 g Ag and 3.0 g S8?

3.5 g Ag2S

How many electrons are shared in a double covalent bond?

4

How many electrons does carbon need to gain in order to obtain a noble-gas electron?

4

What is the total number of covalent bonds normally associated with a single carbon atom in a compound?

4

How many grams of Na2SO4 are needed to prepare 750 mL of a 0.375 M solution?

40 g

How many unshared pairs of electrons are in a molecule of chlorine gas?

6

What is the maximum amount of KCl that can dissolve in 200 g of water? (the solubility of KCl is 34 g/100 g H2O at 20 degrees Celcius)

68 g

___K3PO4 + BaCl2 -->

6KCl+Ba3(PO4)3

What is the mass of Na2SO4 is needed to make 2.5 L of 2.0 M solution? (Na=23 g, S=32 g, O= 16 g)

710 g

Explain what a nonpolar molecule is. Provide an example

A nonpolar molecule has even bonds. The distance between the bonds is equal. Example: CF4

silver + potassium nitrate

Ag +KNO3 --> no reaction

Write the formula for the compoun boron chloride. Why would this name be percieved as incorrect?

BCl3; there is no tri- in front of the chloride

Write the formula for the compound barium oxide

BaO

Name the shapes we studied that automatically make polar molecules. For further bonus, explain why these shapes are automatically polar.

Bent, trigonal pyramidal

1, 6-diminohxane is used to make nylon. What is the empirical formula of this compound if it is 62.1% C, 13.8% H, and 24.1% N?

C3H8N

Calculate the molecular formulas of the compounds having the following empirical formulas and molar masses: C2H5, 58 g/mol; CH, 78 g/mol; and HgCl,236.1 g/mol

C4H10, C6H6, HgCl

The percentage composition of a polymer used for the non-stick surfaces of cooking utensils is 24% C and 76% F by mass. Find the empirical formula.

CF2

Write the correct chemical formula for the compound cadmium phosphate

Cd3(PO4)2

Write the correct chemical formula for the compound cobalt (III) oxide.

Co2O3

Write the correct chemical formula for the compound cobalt (II) oxide.

CoO

Write the formula for the compound cesium telluride.

Cs2Te

Name the compounds CuBr2, SCl2, BaF2. Explain the use or omission of the roman numeral (II) and the prefix di- in each case.

CuBr2- Copper (II) bromide; copper is a stock metal which means that is has more than one charge, so we have to specify which charge it has SCl2- sulfur dichloride; covalent bond, the prefix di- tells us that there are 2 chlorine BaF2- barium fluoride; barium is a non-stock metal which means that it only has one charge

A compound is found to contain 12.95 g N and 37.05 g O. Find the compound's empirical formula. Then, assuming that its actual molar mass is known to be 324 g/mol, find the compound's molecular formula

E: N2O5 M: N6O15

Identify all elements that follow the X-rule format provided by the polyatomic ion rules

Fluorine, Chlorine, Bromine, Iodine

Write a balanced net ionic equation for the following reaction. H3PO4 + Ca(OH)2 --> Ca3(PO4)2 + H2O

H+(aq) + OH-(aq) --> H2O(l)

What is the correct chemical formula for nitrous acid?

HNO2

What is the correect chemical formula for nitric acid?

HNO3

A certain compoun consists of potassium, nitrogen, and oxygen. Hypothesize a possible formula and name for this compound. Explain your reasoning.

KNO2- potassium nitrite KNO3- potassium nitrate

Write the formula of dinitrogen pentoxide

N2O5

Provide the name, formula, and AXE number for a linear molecule

Name- carbon dioxide Formula- CO2 AXE- AX2

Write the formula of diphosphorus tetroxide.

P2O4

Write the formula for the compound rubidium phosphide.

Rb3P

Write the correct chemical formula for the compound tin(II) phosphate

Sn3(PO4)2

Write the formula for the compound strontium sulfide.

SrS

a theory that predicts some molecular shapes based on the idea that pairs of valence electrons surrounding an atom repel each other is called ______________.

VSEPR

What does VSEPR stand for?

Valence Shell Electron Pair Repulsion

Provide the proper formula, name, Lewis structure, and AXE number for a bond experienced between carbo and xenon atoms

Xenon doesn't want to bond; 8 valence electrons

In which of the following is the solution concentration expressed in terms of molarity? a. 10 mol of solute/ 1 L of solution b. 10 g of solute/ 1000 mL of solution c. 10 g of solute/ 1000 g of solution d. 10 mL of solute/ 1 L of solution

a

What is a polar molecule?

a molecule in which the charges are unevenly distributed; H2O, H2S, CH3Cl

The ion formed by an atom of a nonmetal element is a(n) ___________.

anion

In an equation, the symbol for a substance in water solution is ________________.

aqueous (aq)

The mass of the products of the reaction C2H5OH + 3O2--> 2CO2 + 3H2O equals the mass of the reactants because the products are made up of the same _________________ as the reactants.

atoms

In a solution at equilibrium, a. the rate of dissolution is less than the rate of crystallization. b. the rate of dissolution and the rate of crystallization are equal. c. no dissolution occurs d. the rate of dissolution is greater than the rate of crystallization

b

Which of the following substances is less soluble in hot water than in cold water? a. NaNO3 b. CO2 c. NaCl d. KBr

b

Which of the following would be the most concentrated solution? a. 200 g of C12H22O11 b. 100 ppm of C12H22O11 c. 1 mol of C12H22O11 in 1 L of solution d. 1500 ppm of C12H22O11 in water

c

The A in the AXE number of any molecule refers specifically to the _________________.

central atom

A catalyst for a reaction is indicated by a ________ written over the arrow in a chemical equation.

chemical formula

Name the following acid: HClO3

chloric acid

In the compound HCl, the atom of the element _____________ carries a partial negative charge.

chlorine

Name the following acid: HClO2

chlorous acid

Name the compound Co2O3

cobalt (III) oxide

The fact that a compound forms a molecule automatically identifies it as containing __________ bonds.

covalent

Which of the following expresses concentration? a. molality b. parts per million c. molarity d. all of the above

d

The reaction 2HgO(s) --> 2Hg(l) + O2(g) is classified as a(n) _________ reaction

decomposition

Name the compound N2Se4

dinitrogen tetraselenide

Name the compound P2Se5

diphosphorus pentaselenide

In a(n) _________________ reaction, ions of two compounds wxchange places in aqueous solution to form new compounds.

double replacement

Name the following acid: HBr

hydrobromic acid

Name the following acid: HF

hydrofluoric acid

In the compound HCl, the atom of the element ____ carries a partial positive charge.

hydrogen

As the difference between electronegativity values of two elements joined by a bond ____, the degree of the polarity of the bond increases

increases

What is the proper name for FeO2?

iron (IV) oxide

In an ionic bond, the cation is alomst always formed from which type of element?

metal

Name another bond type besides ionic and covalent.

metallic

Provide the name, formula, and AXE number for a bent molecule

name- dihydrogen monoxide formula- H2O AXE- AX2E2

What is the limiting reagent when 150.0 g of nitrogen reacts with 32143 mg of hydrogen in the formation of ammonia?

neither are limiting reagents

If the difference in elctronegativity values between two elements is 0.1 or lower, they will most likely form a(n) ___________ covalent bond.

non-polar

Give the shape of the molecule of SH6

octahedral

Give the proper name of Os(CO3)3

osmium (VI) carbonate

Which energy level is occupied by valence electrons?

outmost energy level

As the difference between electronegativity values of two elements joined by a bond decreases, the less ___________ a bond will become.

polar

If the difference in electronegativity values between two elements if 1.9, they will most likely form a(n) _______________ covalent bond.

polar

An electrically charged group of two or more bonded atoms that function as a single ion is called a(n) _________________ ion

polyatomic

Any compound that contains both covalent and ionic bonds must have at least one _________________ ion.

polyatomic

The reaction Mg(s) + 2HCl(aq) --> H2(g) + MgCl2(aq) is classified as a(n) ______________ reaction.

single replacement

In the chemical reaction 2Cr(s) + 3O2(s) --> 2CrO3(s), two chromium atoms combine with ________________ oxygen atoms

six

Ions that are present in solution in which a reaction is taking place but that do not participate in the reaction are called __________________.

spectator

The reaction 2Mg(s) + O2(g) --> 2MgO(s) is classified as a(n) ____________ reaction.

synthesis

The molecular shape of CBr4 is classified as _____________.

tertrahedral

The molecular shape of CHBr3 is classified as ______________.

tetrahedral

Because of the unique electron configuration of boron, VSEPR theory predicts that the molecular shape of BF3 is classified as ____________________.

trigonal planar

The molecular shape of NH3 is classified as _______________.

trigonal pyramid

The molecular shape of PCl3 is classified as _____________________.

trigonal pyramidal

A covalent bond in which two atoms share three pairs of electrons is called a(n) ____________ bond.

triple

A nonbonding pair of electrons in the valence shell of an atom is called a(n) ______________ pair.

unshared

An electron that occupies the outermost energy level of an atom is known as a(n) _______________ electron.

valence


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