Chemistry 3 Exam Review-1.txt

• c = v • λ
• (p. 270)

c = 3.0 •10⁸ m/s

h = 6.626 •10^-34 J•s

• 1) The principal quantum number (n) indicates size of the orbital. (1, 2, 3, etc.)
• 2) The angular quantum number (l) is related to the shape of the orbital. (from 0 to n-1)
• 3) The magnetic quantum number (m_l) prescribes the orientation of the orbital. (-l through 0 to l)
• 4) The electron-spin quantum number (m_s) describes the spin of the electron itself, not the orbital. (-1/2 or +1/2)

• ∆E = hv
• (p. 274)

• 1/λ = R(1/(n₁)² -1/(n₂)²)
• where n₁ and n₂ are positive integers and n₂ > n₁.
• (p. 277)

• ∆E = E_final - E_initial = -2.18 •10^-18 J(1/(n_final)² - 1/(n_initial)²)
• (p. 279)

λ = h/ mu

• (Use λ = h/ p when finding momentum. Where p is momentum)
• (p. 284)

• ∆x •m∆u ≥ h/4π
• (p. 286)

Order of sublevel energies: s < p < d < f

Electrostatic energy ∂ (cation charge • anion charge) /(cation radius + anion radius) ∂ ∆H_lattice degree

• ∆H_rxn = ∑∆H_{reaction bonds broken} + ∑∆H_{product bonds formed}
• Or
• ∆Hrxn = ∑∆BE_{reaction bonds broken} - ∑∆BE_{product bonds formed}
• (p. 359)

Oscillating, perpendicular electric and magnetic fields moving simultaneously through space as waves and manifested as visible life, x-rays, microwaves, radio waves, and so on. (269)

The number of cycles a wave undergoes per second, expressed in units of 1/second, s^-1.

The distance between any point on a wave and the corresponding point on the next wave, that i, the distance a wave travels during one cycle. (270)

The height of the crest (or depth of the trough) of a wave: related to the intensity of the energy. (270)

The continuum of wavelengths of radiant energy. (271)

The region of the electromagnetic spectrum between the microwave and visible regions. (271)

Radiation in the region of the electromagnetic spectrum between the visible and the z-ray regions. (271)

A phenomenon in which a wave changes its speed and therefore its direction as it passes through a phase boundary. (272)

The phenomenon in which a wave striking the edge of an object bends around it. A wave passing through a list as wide as its wavelength forms a circular wave. (273)

The observation that when monochromatic light of sufficient frequency shines on a metal, an electric current is produced. (274)

A quantum of electromagnetic radiation. (275)

A series of separated lines of different colors representing photons whose wavelength s are characteristic of an element. (276)

In the Bohr model, one of the allowable energy levels of the atom in which it does not release or absorb energy. (277)

The electron configuration of an atom or ion that is lowest in energy. (278)

An electron configuration of an atom or molecule other than the lowest energy state. (278)

A group of instrumental techniques that create an electromagnetic spectrum to measure the atomic and molecular energy levels of a substance. (281)

The line spectrum produced when excited atoms return to lower energy levels and emit photons characteristic of the element. (281)

A procedure for identifying the presence of metal ions in which a granule of a compound or a drop of its solution is placed in a flame to observe a characteristic color. (281)

The spectrum produced when atoms absorb specific wavelengths of incoming light and become excited from lower to higher energy levels. (281)

284

The principle stating that both matter and energy have wavelike and particle-like properties. (286)

The principle stated by Werner Heisenberg that it is impossible to know simultaneously the exact position and velocity of a particle; the principle becomes important only for particle s of very small mass. (286)

An equation that describes how the electron matter-wave changes in space around the nucleus. Solutions of the equation provide allowable energy levels of the H atom. (287)

A region of an orbital where the probability of finding the electron is zero. (293)

The law stating that when the elements are arranged by atomic number, they exhibit a periodic recurrence of properties. (303)

A principle developed by Wolfgang Pauli stating that no two electrons an atom can have the same set of four quantum numbers. The principle arises from the fact that an orbital has a maximum occupancy of two electrons and their spins are paired. (305)

(also screening) The ability of other electrons, especially those occupying inner orbitals, to lessen the nuclear attraction for an outer electron. (306)

The nuclear charge an electron actually experiences as a result of shielding effects dues to the presence of other electrons. (306)

The conceptual basis of a process of building up atoms by adding one proton (and one or more neutrons) at a time to the nucleus and one electron around it to obtain the ground-state electron configurations of the elements. (308)

The principle stating that when orbitals of equal energy are available the electron configuration of lowest energy has the maximum number of unpaired electrons with parallel spins. (309)

An element that occupies the d block of the periodic table; one whose d orbitals are being filled. (313)

315

The elements of the periodic table in which f orbitals are being filled; the lanthanides and actinides. (316)

(also rare earths) The Period 6 (4f) series of inner transition elements, which includes cerium (Ce; Z=58) through lutetium (Lu; Z=71). (316)

The Period 7 elements that constitute the second inner transition series (5f block), which includes thorium (Th; Z=90) through lawrencium (Lr; Z=103). (316)

One-half the distance between the nuclei of adjacent individual atoms in a crystal of an element. (317)

One-half the distance between nuclei of identical covalently bonded atoms. (318)

The energy (in kJ) required to remove completely one mole of electrons from one mole of gaseous atoms or ions. (321)

The energy change (in kJ) accompanying the addition of one mole of electrons to one mole of gaseous atoms or ions. (324)

Able to act as either an acid or a base. (327)

Having the same number of configuration of electrons as another species. (328)

The (n-1)d¹⁰ configuration of a p-block metal atom that has emptied its outer energy level. (328)

The tendency of a species with unpaired electrons to be attracted by an external magnetic field. (330)

The tendency of a species not be attracted (or to be slightly repelled) by a magnetic field as a result of its electrons being paired. (330)

The size of an a ion as measured by the distance between the centers of adjacent ions in a crystalline ionic compound. (332)

Ionic is between a metal and non-metal element where one element transfers electrons to another. Covalent is a bond that shares electrons. And metallic bonding is an idealized type of bonding based on the attraction between metal ions and their delocalized valence electrons. (342-343)

The observation that when atoms bond, they often lose, gain, or share electrons to attain a filled outer shell of eight electrons. (344)

The enthalpy change (always positive) that accompanies a solid ionic compound forming separate gaseous ions. (346)

A series of hypothetical steps and their enthalpy changes needed to convert elements to an ionic compound and devised to calculate the lattice energy. (346)

A law station that the electrostatic force associated with two charges A and B is directly proportional to the product of their magnitudes and inversely proportional to the square of the distance between them. (348)

(also bond enthalpy or bond strength) The enthalpy change accompanying the breakage of a given bond in a mole of gaseous molecules. (353)

An instrumental technique for determining the types of bonds in a covalent molecule by measuring the absorption of IR radiation. (357)

The relative ability of a bonded atom to attract shared electrons. (363)

The difference in electronegativities between the atoms in a bond. (366)

A qualitative description of metallic bonding proposing that metal atoms pool their valence electrons into a delocalized "sea" of electrons in which the metal cores (metal ions) are submerged in an orderly array. (369)

A mixture with metallic properties that consists of solid phases of two or more pure elements, a solid-solid solution, or distinct intermediate phases. (369)