Chemistry Final

In a lab, 20.0 g of ammonia (NH3) are reacted with 20.0 g of hydrogen chloride (HCl) to produce solid ammonium chloride. NH3(g)+HCl(g)→NH4Cl(s) What mass of ammonium chloride is produced? ______ g NH4Cl

29.34

Which of the following is the balanced equation for the combustion of glycerin (C3H8O3) in oxygen?

2C3H8O3 + 7O2 → 8H2O + 6CO2

Which of the following equations is balanced?

2H2+O2→2H2O

Iodine Hydrogen Iron Lithium Boron Beryllium How many of the substances above are held by metallic bonds?

3

N2 + 3H2 → 2NH3 In the reaction above, the coefficient of H2 is ____ . The subscript of H2 is ___, indicating that H2 contains two hydrogen atoms.

3, 2

A certain quantity of magnesium contains 2.84×10^24 atoms of Mg. How many atoms of gold would have the same mass as the magnesium sample?

3.51×10^23 atoms Au

Methane combusts with oxygen through the following reaction: CH4 + 2O2 → CO2 + 2H2O How many grams of carbon dioxide are produced when 16.0 g of methane and 48.0 g of oxygen gas combust? Molar mass of CH4 = 16.0 g/mol Molar mass of O2 = 32.0 g/mol Molar mass of CO2 = 44.0 g/mol

33 g

Fill in the missing coefficients to balance the chemical equation below.

4. NH3 + 5. O2 → 4NO + 6H2O

Fill in the blanks to balance the following chemical equation.

4. P +3. O2→ P4O6

molar mass of iron

55.8 g/mol

2NBr3 + 3NaOH → N2 + 3NaBr + 3HBrO How many NaBr formula units are formed when 50 NBr3 molecules and 57 NaOH formula units react? (Formula units are the equivalent of molecules for ionic compounds e.g. 1 NaBr or 1 NaOH is one formula unit.)

57

The molecular mass of a substance is defined as the mass of how many molecules of the substance?

6.022×10^23

Si + 2Cl2 → SiCl4 What mass of SiCl4 is formed when 10.0 grams of Si and 60.0 grams of Cl2 react? Molar mass of SiCl4 = 169.8 g/mol Molar mass of Cl2 = 70.9 g/mol Molar mass of Si = 28.0 g/mol

60.6 g

Calculate the molar mass of sodium bicarbonate, NaHCO3

84.01 g/mol

What is the mass in grams of 1.50 moles of sodium chloride (NaCl)?

87.7 g

The actual volume of molecules of gas is negligible as compared to the total volume of gas since:

A large volume is occupied by empty spaces

Which of the following is the correct name of HClO4?

Perchloric acid

How do ionic bonds form?

atoms of metallic elements give up electrons to nonmetallic elements

Acids which contain only hydrogen and a single other element are referred to as ______ acids.

binary

What is the name of the acid HClO3HClO3?

chloric acid

The mobile electrons of a pure metal are also called _____ electrons.

delocalized

Collisions between gas particles and between particles and the container walls are _____ collisions because there is no overall loss of kinetic energy.

elastic

A chemical equation is balanced when the number of each type of _____ is the same on both sides of the equation.

element

In a chemical reaction, one of the chemical reactants is present in _____ to make sure that the limiting reagent is completely consumed.

excess

Temperature, according to the kinetic molecular theory, is a measure of intermolecular attraction.

false

The absolute temperature of a gas is a measure of the strength of the intermolecular forces of attraction of that gas.

false

Which of these terms is used to calculate the mass of ionic compounds?

formula mass unit

If the attractive forces in a substance is much less than the molecular motion, then the substance will be in _____ state.

gaseous

In which of the following states of matter would molecules be moving the most?

gaseous

In the Haber reaction shown below, ______ is the limiting reactant if equal moles of each reactant are used. 3H2+N2→2NH3

hydrogen

A gas that completely obeys all of the assumptions of the kinetic-molecular theory is called a(n) _____.

ideal gas

The bond that holds together positive and negative ions is called a(n) _____ bond.

ionic

Which type of bond is formed by the union of nonmetals with metals?

ionic bond

what kind of chemical bond holds NaCl, an ionic crystal together

ionic bond

Which is the correct order for the names and formulas of binary ionic compounds?

metal cation followed by nonmetal anion

Which type of chemical bonding holds elemental iron together?

metallic

Which type of attractive force holds metallic crystals together?

metallic bond

In the covalent compound HI, the number of atoms present in I is represented using the prefix

mono

The Haber process generates ammonia from nitrogen and hydrogen gas through the following chemical equation. N2+3H2→2NH3N2+3H2→2NH3 Which is the excess reagent in the Haber reaction if equal moles of Hydrogen and Nitrogen are used?

nitrogen

In the lattice-like structure of a metal

none of the above

CH3CH2OH+3O2→2CO2+3H2O What would be the limiting reactant in the reaction if 1 mole of oxygen gas and 1 mole of ethanol (CH3CH2OH) reacted with each other?

oxygen gas

Which two elements would NOT be capable of forming an ionic bond?

phosphorous and chlorine

Two charges of the same type will always _____ each other.

repel

Binary molecular compounds are composed of:

two nonmetals

The percentage of partial ionic character depends upon the difference of the _____ of two atoms that join with each other through a covalent bond.

Electronegativity

What is the molar mass of sodium carbonate (Na2CO3)?

106 g/mol

What is the mass of 1.50 moles Cl2?

106.5 grams

Calculate the molar mass of CaCl2.

110.98 g/mol

Calculate the molar mass of iron oxide (Fe2O3).

159.7 g/mol

How many grams are in 0.25 moles of Al(OH)3?

19.50 g

Which coefficient placed before HCl will balance the following equation? Zn+HCl→ZnCl2+H2

2

Which of the following are the missing coefficients of chemical equation: SO2 + ___ H2S → ___ S + 2H2O?

2,3

Calculate the molar mass of aluminum nitrate, Al(NO3)3.

213 g/mol

How many moles are present in 10.0 grams of sodium hydroxide (NaOH)?

0.25 moles

Cl2 + H2 → 2HCl In the reaction above, the coefficient of Cl2 is ___. The subscript of Cl2 is____

1, 2

How many moles of iron(III) oxide are produced from 3.0 moles of oxygen and excess Iron Sulfide as described by the chemical equation below? 4FeS+5O2→2Fe2O3+4SO2

1.2 mol

According to the VSEPR theory, the shape of a covalent molecule depends upon the _____.

All of the above

In the methane molecule CH4, the covalent bonds are non polar since:

All of the above

The number of particles in a mole is known as _____.

Avogadro's number

What is the anion of the ionic compound NaC2H3O2?

C2H3O2-

Choose the name of a CaO compound.

Calcium Oxide

Metal atoms always form the type of ions called _____.

Cations

Matter can neither be created nor destroyed is the law of ________.

Conservation of mass

Choose the name of a CuBr2compound.

Copper (II) Bromide

Which chemical equation is balanced as written?

CuCO3(s)→CuO(s)+CO2(g)

Choose the name for the compound As2O5

Diarsenic Pentaoxide

A water molecule is polar because its hydrogen and oxygen atoms _____.

Do not share electrons equally

In a covalent bond, if the ends have a high electronegativity difference, then the molecule is said to possess a(n) _____.

Electric Dipole

In a polar covalent bond, the atom with a negative charge is less electronegative.

False

The orbital of a non-bonding valence shell electron occupies less space than the orbital which has a bonding pair electron.

False

The VSEPR theory is also known as _____.

Gillespie-Nyholm

What is the formula of phosphorus acid?

H3PO3

Which of the following is the correct name of HClO?

Hypochlorous acid

A bond in which an electron has been transferred from one atom to another is a(n) _____ bond.

Ionic

If the two atoms participating in a bond have an electronegativity difference of 1.9, what type of bond would they be participating in?

Ionic

Which of the following are the correct formulas for potassium oxide and calcium oxide respectively?

K2O; CaO

Which of the following is not a binary compound?

KH2PO4

Choose the name of a LiI compound.

Lithium Iodide

Fill in the blanks according to the chemical reaction below to indicate how many molecules of each substance are present. N2 + 3H2 → 2NH3

Molecules Present (Coefficient- 1 3 2

According to the kinetic molecular theory of gas:

Molecules are in a state of ceaseless and random motion in all directions

What is the cation of the compound NH4HCO3?

NH4+

What is the cation of the compound NH4NO3?

NH4+

What is the cation of the ionic compound Na2SO4?

Na+

Which is the formula for a binary ionic compound composed of iodine and sodium?

NaI

The electronegativity difference for the B-H bond is 0.16. Because this difference is relatively small, this would be considered a _______ covalent bond

Non-polar

A very small electronegativity difference leads to a:

Non-polar covalent bond

In a water molecule, oxygen attracts electrons more strongly than the hydrogens do because an oxygen atom contains more _____ in its nucleus.

Proton

Who did the major work in developing the VSEPR theory?

R.J. Gillespie R.S. Nyholm

The number of electron pairs surrounding an atom is called its _____.

Steric number

What best describes the kinetic energy of two gas particles before and after a collision?

The total kinetic energy of the two particles stays the same.

How is a double bond treated in VSEPR theory compared to a single bond?

There is no difference between a single and double bond.

If the subscript indicating the quantity of a particular element in an ionic formula would be one, the numerical value is omitted instead.

True

For the following reaction: 2Na + Cl2 → 2NaCl There are 2 moles of sodium and 3 moles of chlorine reacting. Which is the limiting reactant?

sodium

What best describes the path of the gas particles in a given sample of gas?

straight path which changes upon collisions with other particles

The ionic compound formed from sodium and chloride ions is commonly known as _____.

table salt

The average speed and kinetic energy of the particles in a gas are proportional to the measured _______ of that gas.

temperature

The average kinetic energy of gas particles depend(s) on the:

temperature of the system

Choose the name for the compound B4H10

tetraboron decahydride

Which atom in a molecule is the focus of VSEPR theory?

the central atom

What is the relationship between the temperature of a gas sample and the kinetic energy of the particles of the gas?

they are directly related