CHM 1310 Lecture Review: Atomic History, Electron Configurations, and Nomenclature

Flashcards covering atomic history, electron configurations, naming covalent and ionic compounds, polyatomic ions, and properties of different bond types.

Ionic Compound Formula Prediction

To predict the formula of an ionic compound, first determine what is known about its constituent elements, such as their expected charges based on their position in the periodic table (e.g., Barium is Ba2+, Chlorine is Cl-).

Naming Covalent Compounds

Rules involve naming the first element, adding a prefix (mono not needed for the first element if only one), naming the second element, using an -ide ending, and adding a prefix for the second element (e.g., H2O is Dihydrogen monoxide).

Transition Metals

Elements that have multiple possible charges, meaning their charges can "transition".

Naming Compounds with Multiple Cation Charges

Involves checking the charges of the elements, then writing the charge of the cation in Roman numerals within parentheses next to the name of the cation (e.g., copper(I) chloride for CuCl, copper(II) chloride for CuCl2).

Ammonium ion

NH4+

Nitrate ion

NO3-

Nitrite ion

NO2-

Hydroxide ion

OH-

Sulfate ion

SO4 2-

Sulfite ion

SO3 2-

Phosphate ion

PO4 3-

Phosphite ion

PO3 3-

Carbonate ion

CO3 2-

Naming with Polyatomic Ions

When naming compounds that include polyatomic ions, name the cation first, followed by the name of the polyatomic ion (e.g., KNO3 is potassium nitrate).

Diatomic Elements

Elements that bond to themselves in their natural states (H2, N2, O2, F2, Cl2, Br2, I2).

Atomic Mass Calculation

Calculated using the equation: Atomic mass = (mass of isotope 1)(% abundance) + (mass of isotope 2)(%abundance) + …etc.

Covalent Bond

A bond where two atoms share electrons, with their orbitals overlapping; occurs between two non-metals.

Properties of Covalent Compounds

Attractive forces between molecules are weak, leading to low melting temperatures.

Ionic Compounds

Compounds formed when electrons are completely transferred between a metal and a non-metal, creating charged ions.

Ion

A form of an atom that has gained or lost electrons, resulting in an overall electrical charge.

Cation

A positively charged ion formed when an atom loses electrons (e.g., Na+).

Anion

A negatively charged ion formed when an atom gains electrons (e.g., O2-).

Naming Ionic Compounds

Write the name of the cation first, then the name of the anion with an -ide suffix (e.g., NaCl is sodium chloride).

Alkali metals

Elements in Column 1 of the periodic table, typically forming +1 ions.

Alkaline earth metals

Elements in Column 2 of the periodic table, typically forming +2 ions.

Aluminum ion charge

+3.

Column 15 ion charge

-3.

Column 16 ion charge

-2.

Halogens

Elements in Column 17 of the periodic table, typically forming -1 ions.

Noble gases

Elements in Column 18 of the periodic table, typically having a 0 charge (stable electron configuration).

Silver ion charge

Ag+, +1.

Zinc ion charge

Zn2+, +2.

Cadmium ion charge

Cd2+, +2.

Properties of Ionic Bonds

Ionic bonds form crystal lattices, which allow the structure to be hard and rigid, resulting in very high melting points.

Leucippus and Democritus' atomic theory

Proposed in 440 B.C. that matter is made of small, hard, indivisible particles called atoms.

Aristotle's view on matter

Believed that matter divides infinitely and no indivisible particles exist, opposing the early atomic view.

Antoine Lavoisier's Experiment (1785)

Heated mercury(II) oxide in a sealed system, discovering that the total mass before heating equals the total mass after, demonstrating the law of conservation of mass.

Law of Conservation of Mass

Mass is neither created nor destroyed in a chemical reaction, but merely changes form.

Dalton's Atomic Theory Tenet 1

All matter is made up of tiny, indivisible particles called atoms (later found to be partially false).

Dalton's Atomic Theory Tenet 2

Atoms cannot be created, destroyed, or transformed into other atoms in a chemical reaction (later found to be partially false).

Dalton's Atomic Theory Tenet 3

All atoms of a given element are identical (later found to be partially false due to isotopes).

Dalton's Atomic Theory Tenet 4

Atoms combine in simple, whole-number ratios to form compounds (explains the law of conservation of mass by rearrangement of atoms).

Cathode Ray Tubes

Used by J. J. Thompson in 1897 to discover electrons; voltage applied resulted in visible rays deflected by magnets, indicating charged particles.

J. J. Thompson's Discovery (1897)

Calculated the size of cathode ray particles, determined they were 1/1000 of any known element, and concluded they were negatively charged particles called electrons.

Electrons

Negatively charged subatomic particles that are part of an atom, possessing a negligible mass.

Plum Pudding Model

Thompson's proposed atomic model where the atom consists of a positively charged matrix with negatively charged electrons floating within it.

Ernest Rutherford's Gold Foil Experiment (1909)

Projected a beam of alpha rays through a thin film of gold, leading to the discovery of the atomic nucleus and protons.

Gold Foil Experiment Conclusion 1 (Empty Space)

Most alpha particles went directly through the film, leading to the conclusion that the atom must be mostly empty space.

Gold Foil Experiment Conclusion 2 (Positive Deflection)

Some alpha particles were deflected slightly, indicating they were pushed off course by something that is also positively charged.

Gold Foil Experiment Conclusion 3 (Dense Source)

Rarely, an alpha particle was deflected directly backwards, indicating it directly hit a very dense source within the atom.

Nucleus

The very dense, positively charged center of an atom, discovered by Ernest Rutherford.

Protons

Positively charged subatomic particles discovered by Rutherford, located in the nucleus.

Principal Quantum Number (n)

Represents the location of the energy level in an atom, determined by the row on the periodic table (with transition metals as an exception).

s orbital

A spherical electron orbital where the probability of finding an electron is greatest at the center.

p orbital

A dumbbell-shaped electron orbital with probability greatest near the node at the center, existing as three dumbbells along the x, y, and z axes.

Electron Orbitals

Regions of space around the nucleus that express the probability of finding an electron in a certain location.

Electron Configuration

A system devised to categorize and identify the distribution of electrons within the orbitals of an atom.

Electron Configuration "Big Number"

Represents the energy level, equal to the row on the periodic table where this orbital is found.

Electron Configuration "Letter"

Represents the type of orbital (s, p, d, f).

Electron Configuration "Exponent"

Represents the number of electrons in that specific orbital; the sum of all exponents equals the total number of electrons in the element.

s orbital maximum electrons

Can hold a maximum of 2 electrons.

p orbital maximum electrons

Can hold a maximum of 6 electrons.

d orbital maximum electrons

Can hold a maximum of 10 electrons.

Noble Gas Configuration

A shorthand notation for electron configuration where part of the configuration is substituted for the symbol of a noble gas in brackets, preceding the remaining electron configuration (e.g., [Ar]4s2 for calcium).