Chemistry: Isotopes, Atomic Structure, and Bonding - Practice Flashcards

A set of practice questions covering isotope theory, atomic structure, periodic trends, ionic and molecular naming, and basic stoichiometry concepts from the lecture notes.

What is the purpose of the Lecture Slide Quizzes described in Page 1?

They are for personal knowledge checks and are not for credit.

When are ALEKS assignments due according to the notes?

Wednesdays at 11:59 pm CST.

Where are Lab Materials typically located in the course module?

In D2L under Content → Materials → Laboratory Materials submodule (per lab).

What is the due time and number of attempts for the Pre-lab Quiz on D2L?

Due during the week on Tuesdays at 11:59 pm CST, with 2 attempts.

What must be completed to release the Post-lab Quiz according to the notes?

The Laboratory Assignment (Assessments-Assignments) from the following week.

What does STM stand for, as mentioned in the notes?

Scanning Tunneling Microscopy.

Where is the mass of the atom primarily located?

In the nucleus.

What is the relationship between the charge of a proton and the charge of an electron?

They are equal in magnitude but opposite in sign.

What is the atomic mass unit (amu) defined as?

One-twelfth the mass of a carbon-12 atom.

How is the mass number A related to protons and neutrons?

A = number of protons + number of neutrons.

How is the atomic number Z defined?

Z equals the number of protons (and, in a neutral atom, the number of electrons).

What do isotopes have in common and how do they differ?

They have the same atomic number Z but different mass numbers A.

How do you calculate the number of neutrons from A and Z?

Neutrons = A − Z.

What is the formula to calculate the average atomic mass from isotopes?

Sum of (fractional abundance × isotopic mass) for all isotopes.

What is meant by the percent abundance of an isotope?

The percentage of a given isotope in a natural sample: (number of atoms of that isotope / total number of atoms) × 100.

What is the relationship between natural abundance and atomic weight?

Atomic weight is the weighted average of isotopic masses based on their natural abundances.

What is the formula for percent abundance in a multi-isotope element?

Percent abundance = (number of atoms of isotope / total number of atoms) × 100.

What is a polyatomic ion?

An ion composed of two or more atoms.

What suffix endings are used for oxoanions with more oxygen vs. less oxygen, and what mnemonic helps remember this?

-ate for more oxygen, -ite for less; mnemonic: "I ate more oxygens."

What forms exist for oxoanions when there are four possibilities, and what are their names?

Per-…-ate (most O), -ate, -ite, and hypo-…-ite (fewest O).

Give examples of oxoanions and their suffixes (examples from the notes).

Sulfate (SO4^2−), Sulfite (SO3^2−); Nitrate (NO3^−), Nitrite (NO2^−).

How are binary ionic compounds named?

Name the cation (usually the metal) first; name the anion second, changing the ending of the anion to -ide.

How is the charge of transition metal cations indicated in naming?

With Roman numerals in parentheses after the metal, e.g., Cu^2+ is Cupric, Cu^+ is Cuprous.

What method is used to determine ionic compound formulas from charges?

The cross-and-drop (criss-cross) method.

Which formula corresponds to Iron(III) nitrate?

Fe(NO3)3.

What is a hydrated ionic compound and what does 'n' represent in MX·nH2O?

A compound with a definite amount of water; n is the number of water molecules per formula unit.

What is a molecule, and what distinguishes homonuclear and heteronuclear diatomic molecules?

A molecule is a group of at least two non-metal atoms held by covalent bonds; homonuclear diatomic contains two atoms of the same element (e.g., O2), heteronuclear diatomic contains two different elements (e.g., CO).

Name the seven diatomic molecules that are naturally found as diatomic elements.

H2, N2, O2, F2, Cl2, Br2, I2.

What prefixes are used for naming binary nonmetal molecular compounds, and what do they mean?

Mono-, di-, tri-, tetra-, penta-, etc.; they indicate the number of atoms of each element in the molecule.

What is an empirical formula, and how does it differ from a molecular formula?

Empirical formula shows the smallest whole-number ratio of elements; molecular formula shows the actual number of atoms in a molecule.

What is the role of the variable n in empirical vs. molecular formulas?

n represents the number of repeat units in the molecule; used in the context of empirical vs. molecular formulas.

What is the correct name for H2O in binary molecular compound naming?

Water.

What is the correct formula for calcium hydroxide?

Ca(OH)2.

What is the correct formula for potassium sulfate?

K2SO4.

Which formula is not correct for a polyatomic ion-containing compound: Mg(NO3)3, NH4CO3, NaClO4, or Al2(SO4)3?

Mg(NO3)3 is not correct.

What kind of change is typically shown by comparing observations like color, odor, or phase changes in a reaction?

Chemical change (as opposed to physical change), though some situations can show both.