CHM1025 - Exam 2 Study Guide Cartes | Quizlet

NH4+

ammonium (cation)

H3O+

hydronium (cation)

C2H3O2- (CH3COO-)

acetate (anion)

N3-

azide (nitride, anion)

OH-

hydroxide (anion)

O2^2-

peroxide (anion)

CO3^2-

carbonate (anion)

HCO3-

hydrogen carbonate (bicarbonate, anion)

CrO4^2-

chromate (anion)

Cr2O7^2-

dichromate (anion)

CN-

cyanide (anion)

BrO4-

perbromate (anion)

BrO3-

bromate (anion)

BrO2

bromite (anion)

BrO-

hypobromite (anion)

ClO4-

perchlorate (anion)

ClO3-

chlorate (anion)

ClO2-

chlorite (anion)

ClO-

hypochlorite (anion)

IO4-

periodate (anion)

IO3-

iodate (anion)

IO2-

iodite (anion)

IO-

hypoiodite (anion)

MnO4-

permanganate (anion)

NO3-

nitrate (anion)

NO2-

nitrite (anion)

SO4^2-

sulfate (anion)

SO3^2-

sulfite (anion)

HSO4-

hydrogensulfate (anion)

HSO3-

hydrogensulfite (anion)

PO4^3-

phosphate (anion)

PO3^3-

phosphite (anion)

HPO4^2-

hydrogenphosphate

H2PO4-

dihydrogenphosphate (anion)

HPO3^2-

hydrogenphosphite (anion)

H2PO3-

dihydrogenphosphite

Properties of Ionic Compounds

crystalline solid, hard, brittle solid, very high melting point, very high boiling point, high density, strong electrolyte in aqueous solution, electrical conductivity good when compound is molten.

Properties of Molecular Compounds

gas, liquid, solid, soft solid, low melting point, low boiling point , low density, weak electrolyte or non-electrolyte in aqueous solution, electrical conductivity poor in pure form.

Monatomic Ion

An ion with a single atom.

How are monatomic ions named?

Monatomic anions are named as the first part of the element name (called the root of the name) and -ide is added as a suffix. e.g. S^2-, sulfide ion. the charges on common monatomic ions of many main group elements correlate with the elements' position in the periodic table.

O^2-

oxide ion

Na+

sodium ion

N^3-

nitride ion

Al^3+

aluminum ion

Mg^2+

magnesium ion

Cl-

chloride ion

K+

potassium ion

F-

fluoride ion

Polyatomic ion

Polyatomic ion is an ion containing two or more atoms, usually of more than one element.

Oxyanions

One of the most common compounds, combinations of oxygen with a nonmetal, although some contain metals.

Electromagnetic radiation

A form of energy produced when charged particles move or vibrate relative to each other; electromagnetic radiation exists as waves.

Photons

A small increment or packet of electromagnetic energy (often visible light). We an think of a photon as a packet of light.

Electromagnetic spectrum

All forms of electromagnetic energy, ranging from low-energy waves (TV and radio) to visible light to high-energy waves such as gamma rays.

Visible spectrum

The narrow range of electromagnetic energy that we perceive as light. We can see that it is made up of the colors of the rainbow: red, orange, yellow, green, blue, and violet.

Wavelength

Symbolized by the greek letter lambda. It is the distance from a point on one wave to the same point on the next wave. Wavelength is typically measured in meters or nanometers (recall that 1nm= 10^-9 m). The longer the wavelength, the lower the frequency.

Frequency

Symbolized by the greek letter nu. It is the number of waves that pass through a point in one second.

Hertz

A frequency of one wave cycle per second. The units corresponding to hertz are written as Hz, 1/s, or sometimes as s^-1.

What is the relationship between wavelength and frequency?

c= λν, where c is the speed of light (in a vacuum it is equal to 3.00 x 10^8 m/s.

How can we relate the energy of a single photon to its frequency?

E= hν, where E is the energy (measured in joules), ν is the frequency, and h, which is referred to Planck's constant, has a value of 6.63 x 10^-34 J . s.

How can we relate the energy of a single photon to its wavelength?

E =hc/ λ, where E is the energy (measured in joules), h is Planck's constant, c is the speed of light, and λ is the wavelength

Line spectra

A pattern of light energies called spectral lines; they are formed when gas-phase elements release energy. Each element has a characteristic line spectrum.

Bohr Model

(1913) An early model of atomic structure that treated the atom like a tiny solar system, with the nucleus at the center, and the electrons orbiting the nucleus. Niels Bohr suggested that electrons orbiting close to the nucleus are lower in energy than those that are farther away, and he posited that only certain orbits, or energy levels, are "allowed." He also proposed that electrons can jump from one energy level to another. He theorized that when an electron absorbs light, it jumps to a higher energy level. When it drops to a lower energy level, it releases that energy as light.

Quantum model

The modern description of electronic behavior that treats electrons as particles and as waves.

Uncertainty principle

An idea introduced in 1927 by scientist Werner Heisenberg. It states that it is impossible to know the exact velocity and location of a particle; this principle becomes important when studying electrons .

Principal quantum number

An integer that identifies the energy level an electron occupies. The lowest energy level (level 1) lies closest to the nucleus. Higher energy levels (2, 3, 4, etc.) lie farther from the nucleus. Each energy level can hold a maximum number of electrons. Higher energy levels can hold more electrons than lower energy levels.

Sublevels

A set of electron orbitals that occurs in an electron energy level; the four main sublevels are s, p , d, and f. Energy levels and sublevels are sometimes referred to as energy shells and subshells, respectively.

Orbital

A region where electrons are most likely to be found, each orbital can hold up to two electrons. An s sublevel contains 1 orbital; a p contains 3, a d contains 5, and an f contains 7.

Spin

Each orbital can hold up to two electrons. Electrons have a tiny magnetic field, called spin. When electrons pair together in orbitals, their spins orient in opposite directions. An orbital is filled if it contains two paired electrons.

Energy level 1: s sublevel

A sublevel that contains one orbital and can hold up to two electrons; the s sublevel is present in every energy level. Its orbital is shaped like a sphere.

Energy level 2: s and p sublevels

The 2s sublevel is spherical in shape, but it lies farther from the nucleus than the 1s sublevel. The p sublevel contains three orbitals an can hold up to 6 electrons; the p sublevel is present in energy levels 2 and higher. Its orbitals have a shape similar to an infinity symbol.

Energy level 3: s, p, and d sublevels

The d sublevel contains 5 orbitals and can hold up to 10 electrons; the d sublevel is present in energy levels 3 and higher.

Energy level 4: s, p, d, and f sublevels

The f sublevel contains seven orbitals and can hold up to 14 electrons; the f sublevel is present in energy levels 4 and higher.

Order of energy levels and sublevels

1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p

Electron configurations

The number of electrons in each energy level and sublevel. ex. 1s^1. In this notation, the 1s means that energy level 1, sublevel s, is occupied. The superscript 1 indicates that one electron resides in this orbital.

Hund's Rule

If empty orbitals of the same energy are available, electrons will singly occupy orbitals rather than pair together.

Valence level

The highest-occupied electron energy level in an atom. As a general rule, atoms hold up to eight electrons in their valence level.

Octet rule

The principle that an atom is stabilized by having its highest-occupied (valence) energy level filled. If an atom has eight electrons (an octet) in its valence shell, the s and p sublevels are completely filled.

Noble Gas Notation

An abbreviated electron configuration of an element in which filled inner shells are represented by the symbol of the preceding noble gas in brackets. For example, 1s^2 2s^2 2p^6 s the configuration of neon. We represent it by enclosing the symbol for neon in square brackets: [Ne].

How is the periodic table organized based on electronic structure?

Elements in the first row (H and He) have electrons only in energy level 1, elements in the second row (Li through Ne) have electrons in energy level 2, and so forth. For any atom, we can determine its highest-energy electron shell from the row it occupies on the periodic table. Main-group number gives the valence electrons.

Lewis dot symbols

A method of representing the valence structure of an atom or ion that involves using dots around the atomic symbol to indicate valence electrons.

Cation

A positively charged ion. Main-group metals fulfill the octet rule by losing electrons and forming cations. All of the alkali metals (metals in group 1A of the periodic table) lose one electron to form +1 ions. Each of the alkali earth metals (group 2A) loses two electrons to form +2 ions.

Naming cations

Metal cations are given the same name as the neutral metal. if an atom can form more than one cation, use Roman numerals after the atom name to specify the charge.

Anions

A negatively charged ion. Most nonmetals gain electrons to form anions. The halogens fluorine, chlorine, bromine, and iodine form -1 ions. Oxygen, sulfur, and the atoms below them are called chalcogens; they form -2 ions. 5A elements form ions with a charge of -3.

Naming anions

When an atom gains electrons, we name the resulting anion by changing the end of the atom name to -ide. Ex. Chloride ions, oxide ions, and sulfide ions.

N^3-

Nitride

P^3-

Phosphide

O^2-

Oxide

S^2-

Sulfide

F^-

Fluoride

Cl^-

Chloride

Br^-

Bromide

Polyatomic ions

A group of covalently bonded atoms with an overall charge.

Naming polyatomic ions

Oxyanions- anions containing oxygen. These are named by adding the suffix -ate to the root of the element. If elements form more than one oxyanion, we use -ate to indicate the ion with more oxygen atoms present, and -ite to indicate the ion with fewer oxygen atoms. Chlorine forms 4 oxyanions. We use per- to indicate the largest number of oxygen atoms and hypo- to indicate the least number of oxygen atoms.

Ionic bond

A force of attraction between oppositely charged ions.

Ionic compound

A compound of oppositely charged ions. The compounds formed between metals and nonmetals are ionic compounds.

Ionic lattice

A tightly packed array of alternating positive and negative charges; the characteristic arrangement of ions in an ionic solid.

Chemical formula

A representation of the type and amount of each element present in a compound.

Empirical formula

How ionic compounds are represented. It is a chemical formula that gives the smallest whole-number ratio of atoms in a compound. Subscripts written after each atom indicate the number of that atom present.

Formula unit

In ionic compounds, the smallest number of ions necessary to form a compound; the combination of atoms described by an empirical formula.

Naming ionic compounds

We give the cation name followed by the anion name. For transition metals with more than one possible charge, it is important to include the charge of the ion in parentheses with the name.