Chemistry

• 3.00 x 10^8m/s
• c

• Alkali metals
• chemically reactive (more reactive than group 2)

• Alkali Earth metals
• chemically reactive

• halogen
• highly reactive

• noble gases
• extremely non reactive

2 sets: Lanthanide and Actinide

Decreases: because increasing number of protons = increase charge = stronger pull of e- cloud = smaller atomic radius

increases: more e- shells are added making radius bigger

• neutral atom is smaller than positive ion: because has more electron shells
• negative ion is bigger than neutral ion: because more electrons in outer shell = increase repulsion between e- = creating larger radius

• energy required to remove and electron from a gaseous atom
• kJ/mol
• High IE = strong hold on e- (less likely to form pos. ions)
• Low IE = weak hold on e- (more likely to form pos. ions)

increased IE: nuclear charge increases and has more pull on valence electrons

Decreased IE: greater distance between valence electrons and nucleus, so less energy required since pull isnt as strong

atoms tend to gain, lose, or share e- to acquire full set of 8 valence electrons

indicates relative ability of atoms to attract electron in chemical bond

*greater EN = more attraction of electrons in bond

increases as move across period and decreases as moves down group

• energy increases with increasing frequency
• wavelength and frequency are related; as one increases the other decreases
• purple = highest energy (high frequency)
• red = lowest energy (low frequency)

• energy needed to break 1 mole of an ionic compound into its gaseous ions
• measured in kJ/mol
• breaking down ions requires energy
• forming compounds releases energy
• High LE = strong attraction between positive and negative ions
• Low LE = weak attraction

• sulfate: SO₄^2-
• Carbonate: CO₃^2-
• Nitrate: NO₃^-
• Hydroxide: OH^-
• Ammonium: NH₄^-
• Copper: Cu ¹⁺ - Cu²⁺
• Iron: Fe²⁺ - Fe³⁺
• Lead: Pb²⁺ - Pb⁴⁺
• Silver: Ag¹⁺
• Zinc: Zn²⁺

LE decreases: because gets easier to break down structure because attraction of nucleus to electron is very low

• ionic radii: big ions have less attractive force between ions than small ions
• Magnitude of ionic change: the higher the charge of the ions, the greater the attraction, and the higher the LE energy

• metal + metal
• rep. particle = atoms

• ion + ion
• rep. particle = formula units

• matal + nonmetal
• rep. particle = molecules

atomic mass expressed in grams / 1 mole

(mass) x (% abundance) = ____amu

• 1L = 1000 mL = 1000cm³
• 1mL = 1cm³
• 1mi = 5280ft

(mass of element) / (total compound mass) x 100 = _____ % (E)

atomic number = number of protons = number of electrons

number of neutrons = mass number - atomic number

(true value - experimental value) / true value x 100 = the error (low # = good & high # = bad)

• mass = density x volume
• density = mass / volume
• volume = mass / density

1.0g / ml