Chemistry Unit 3

This set of flashcards covers key concepts related to molecules, compounds, nomenclature, chemical formulas, and related definitions from the lecture notes.

Covalent bonds involve __ of electrons between atoms.

sharing

Ionic bonds involve __ of electrons from one atom to another.

transfer

Molecular compounds contain covalent bonds between __ atoms.

non-metal

The chemical formula for glucose is __.

C6H12O6

The __ formula shows the simplest whole number ratio of atoms present in a compound.

Empirical

The __ formula shows the actual number of atoms present of each element in a molecule.

Molecular

A __ formula represents the order in which atoms are bonded together in a molecule.

Structural

Condensed structural formulas are written on a __ line.

single

Ionic compounds typically consist of __ and non-metals.

metals

A formula unit is the smallest electrically neutral collection of __.

ions

Organic compounds typically consist of carbon and __.

hydrogen

Binary ionic compounds are formed between __ elements.

two

In naming binary ionic compounds, the order is __ name followed by anion name.

cation

Transition metals may form several types of __.

cations

The most common polyatomic ion that carries a +1 charge is __.

ammonium (NH4+)

The suffix __ is used for the ion with fewer oxygen atoms in a family of oxyanions.

-ite

In naming acids with no oxygen, the name consists of prefix hydro-, nonmetal root plus suffix __.

-ic

Combustion analysis is used to determine the amounts of and in a combustible organic compound.

carbon, hydrogen

Acids that contain oxygen are known as __.

oxoacids

The molecular mass of a compound is the sum of the __ of the atoms in a molecule.

atomic masses

To calculate the mass percent of an element in a compound, you can use the formula: (mass of element in formula)/(mass of compound) × 100%

The empirical formula for the compound if it produces 165g carbon, 27.8g hydrogen, 220.2g oxygen is __.

CH2O

In binary covalent compounds, the second element is named as if it were an __.

anion

The mass percent composition is the mass percentages of __ elements in a compound.

individual

Covalent bonds involve \\ of electrons between atoms.\n\n

sharing\n\n

Ionic bonds involve \\ of electrons from one atom to another.\n\n

transfer\n\n

Molecular compounds contain covalent bonds between \\ atoms.\n\n

non-metal\n\n

The chemical formula for glucose is \\.\n\n

C6H12O6\n\n

The \\ formula shows the simplest whole number ratio of atoms present in a compound.\n\n

Empirical\n\n

The \\ formula shows the actual number of atoms present of each element in a molecule.\n\n

Molecular\n\n

A \\ formula represents the order in which atoms are bonded together in a molecule.\n\n

Structural\n\n

Condensed structural formulas are written on a \\ line.\n\n

single\n\n

Ionic compounds typically consist of \\ and non-metals.\n\n

metals\n\n

A formula unit is the smallest electrically neutral collection of \\.\n\n

ions\n\n

Organic compounds typically consist of carbon and \\.\n\n

hydrogen\n\n

Binary ionic compounds are formed between \\ elements.\n\n

two\n\n

In naming binary ionic compounds, the order is \\ name followed by anion name.\n\n

cation\n\n

Transition metals may form several types of \\.\n\n

cations\n\n

The most common polyatomic ion that carries a +1 charge is \\.\n\n

ammonium (NH_4+)\n\n

The suffix \\ is used for the ion with fewer oxygen atoms in a family of oxyanions.\n\n

\-ite\n\n

In naming acids with no oxygen, the name consists of prefix hydro-, nonmetal root plus suffix \\.\n\n

\-ic\n\n

Combustion analysis is used to determine the amounts of ** and in a combustible organic compound.\n\n

carbon, hydrogen\n\n

Acids that contain oxygen are known as \\.\n\n

oxoacids\n\n

The molecular mass of a compound is the sum of the \\ of the atoms in a molecule.\n\n

atomic masses\n\n

To calculate the mass percent of an element in a compound, you can use the formula: (mass of element in formula)/(mass of compound) × 100%\n\n

The empirical formula for the compound if it produces 165g carbon, 27.8g hydrogen, 220.2g oxygen is \\.\n\n

CH2O\n\n

In binary covalent compounds, the second element is named as if it were an \\.\n\n

anion\n\n

The mass percent composition is the mass percentages of \\ elements in a compound.\n\n

individual\n\n

The prefix penta- in a binary covalent compound indicates there are \\ atoms of that element.

five

Calculate the molecular mass of ammonia (NH_3). (Atomic masses: N = 14.01 amu, H = 1.01 amu)

R\text{MM for } NH3 = 1(14.01) + 3(1.01) = 14.01 + 3.03 = 17.04 \text{ amu}

When is a compound's molecular formula identical to its empirical formula?

When the molecular formula cannot be simplified to a smaller whole-number ratio of atoms.

The polyatomic ion with the formula SO4^{2-} is called \\_.

sulfate

If an oxyanion ends in \-ite, the corresponding oxoacid name will end in \\ and will \\ a hydro- prefix.

-ous, not include

A compound is found to contain 85.63\% carbon and 14.37\% hydrogen by mass. What is its empirical formula? (Atomic masses: C = 12.01 g/mol, H = 1.01 g/mol)

Assume 100g sample: 85.63g C and 14.37g H.\nMoles C: 85.63g / 12.01 g/mol = 7.13 mol\nMoles H: 14.37g / 1.01 g/mol = 14.23 mol\nDivide by smallest: C: 7.13 / 7.13 = 1; H: 14.23 / 7.13 = 2\nEmpirical Formula: CH_2