Gen Chem 2 Exam 6

metals

solid at room temperature, lustrous, malleable, conductive of hear and electricity

transition metals

occupy the d and f blocks of the periodic table

Metalloids

have properties of both metals and nonmetals (semiconductors, shiny, brittle solids)

Nonmetals

brittle dull, poor conductors or nonconductors

A. metals, B. nonmetals, C. metalloids

Label A, B, and C by element classification

periods

— are rows

groups

— are columns

coordination compound

composed of coordination complex

coordination complex

the product of a Lewis acid-base reaction in which neutral molecules or anions bond to the central metal atom (or ion) by coordinate covalent bonds

ligand

the Lewis base (neutral/negative molecule)

central metal atom

the Lewis acid

coordinate covalent bond

one atom supplies both shared electrons

donor atom

the atom that supplies the shared electrons

complex ion

coordination complex that carries a charge

coordination sphere

the central metal plus its attached ligands (indicated by [] in the chemical formula)

coordination number

the number of donor atoms bonded to the central metal atom

A. OH^- B. Fe²⁺ C. O D. 4

	Lewis base (ligand)	Lewis acid (central metal)	Donor atom	Coordination number
[Fe(OH)4]2-	A. ________	B. ________	C. ________	D. ________

Alkali, 1, 1+, largest, lowest, fog penetration, batteries

Group 1: — metals: # valence electron, # typical charge, classified as metals (except H), have the — atomic radii and the — ionization energy, common uses: Na is used for — — street lights, Li is used in —

alkaline, 2, 2+, reducing, ionic, fireworks, chalk

Group 2: — Earth Metals: # valence electron, # typical charge, classified as metals, strong — agents, form — compounds, common uses: —, airplanes, —, paint, toothpaste

1, 2+, transition metals, decreases, amalagams

Group 12: # valence electron, # typical charge, classified as — —, similar behavior to group 2 but reactivity trend — as you go down the group, common applications: —

amalagam

alloy of Mercury (Hg) and some other metal, useful for panning for gold and dental fillings

3, 3+, metal, amphoteric, basic, semiconductor, commercial

Group 13: # valence electron, # typical charge, classified as —, forms oxides that can be — or —, B is a —, Al is used in many industrial, transport and — products

4, 4+, metal, allotropes, life

Group 14: # valence electron, # typical charge, classified as —, produces several —, common uses carbon forms organic compounds necessary for all —

allotropes

same element in same physical state with different physical and chemical properties (ex carbon: graphite vs diamonds)

inert pair effect

the formation of a stable ion with an oxidation state 2 lower than expected for the group

5, 5+ to 3-, variety, increases, protein, DNA, batteries

Group 15: # valence electron, # typical charge, has a — of elemental classes, metallic character — as you go down the group, N and P are essential for — and —, also produces alloys used in —

Group 16:

7, 1-, nonmetals, diatomic, increases, halides

Group 17: Halogens: # valence electron, # typical charge, classification —, exist as — molecules, highly reactive, Van der Waals forces — down the group, common uses: binary —

Nobel gases, 8, 0, nonmetals, reactive, electric

Group 18: — —: # valence electron, # typical charge, classification —, least — elements, very low melting points, common uses: glow in characteristic colors when an — current is applied

protons

positively charged molecules in the nucleus

neutrons

neutral charge molecules in the nucleus

electrons

negatively charged molecules surrounding the nucleus

₆¹⁶C, 10

1) Write the notation of the following isotopes using the format: _Z^XA. 2) State the number of neutrons in each nuclide.

Carbon-16

convert amu to kg, use E=mc², Convert J to eV

to find the nuclear binding energy when given the mass defect: ST1 —-, St2 —-, St3—

atomic number

the number of protons in an atom (Z in _Z^AX)

mass number

the number of protons and electrons in an atom (A in _Z^AX)

alpha particle

He nuclei consisting of 2p⁺ and 2n⁰

beta particle

an electron

positron

particles with same mass as an electron but with 1 unit of positive charge

proton

nuclei of H atoms

neutron

particles with a mass approximately equal to that of a proton but with no charge

gamma ray

very high energy electromagnetic radiation

alpha decay

the emission of an alpha particle from the nucleus (you get some element plus and alpha particle/He)

beta decay

the conversion of a neutron into a proton and a beta particle (you get some element plus a -1 beta)

gamma emission

when a nuclide is formed in an excited state and then decays to its ground state with the emission of a gamma ray (same element plus gamma)

positron emission

when you get an element and a positron (+1e or +1 beta)

electron capture

when you have an electron that combines with a proton to produce a new element

decay

half-life of a radioisotope is the time required for half of the atoms in the sample to —

dispose, replaced

radioisotope half-lives are useful for knowing how long a substance will be radioactive and when it is safe to —of, it is also useful for determining how long it is available before it must be —

transmutation

the conversion of one nuclide into another

radioactive, manipulated

transmutation can occur naturally through — decay or be — in a laboratory setting

nuclear fission

breaking of a large nucleus into smaller pieces, releasing large amounts of energy

nuclear fusion

the process of converting lighter nuclei to heavier nuclei

non-ionizing radiation

lower-frequency energy waves that cause particles to speed up, producing heat (microwaves, radiowaves)

ionizing radiation

higher frequency energy waves that break bonds and remove electrons, disrupting the function of biomolecules (used to treat cancer)

Raydon-222

radiation that is found naturally in soil and can accumulate in basements

cation, anion, ligand, latin

Rules for naming complexes:

1. if the coordination compound is ionic, name the — first and the — second

2. name the — first then the central atom

3. if more than one ligand is present, a numerical prefix is added to indicate the number of ligands used

4. when the complex is a cation the oxidation state of the central metal is indicated in its name using roman numerals

5. when the complex is an anion the name of the central atom is given the suffix -ate and given the oxidation number in its name

6. if the common English name is clumsy use —