chemfinal

• Physical: chemical bonds are not broken can be observed
• Chemical: can only be observed when a substance is changed into another substance

• Intensive: independent of the amount of the substance that is present. Ex: density, boiling pt, etc.
• Extensive: depend upon the amount of the substance is present. Ex: mass, volume, energy, etc

• Physical: changes in matter that do ot change the compostition of a substance Ex: temp, volume, changes in states
• Chemical: result in new substances E: combustion, oxidation, decomposition

• D: uses differencs in the boiling points of substances to spearate a homogeneous mixture into its components
• F: substances are separated from liquids and solutions
• C: separates substances on the basis of differences in solubility in a solvent

• meters
• s²
• K
• mole

• 9/5(C)+32
• 5/9(F-32)
• C+ 273.15

• Accuracy: proximity of a measurement to the true value of a quantity
• Precision: proximity of several measurements to each other

• Rutherford
• james Chadwick

• periods
• groups

• alkali metals
• alkali earth metals
• chalcogens
• halogens
• noble gases

• Hydrogen
• Nitrogen
• Oxygen
• Flourine
• Chlorine
• Bromine
• Iodine

• Combination
• Decomposition
• Combustion

• T: calculate
• A: what actually comes out

• E: dissociates into ions when dissolved in water
• N: dissolves in water but do not dissociates into ions

• Hydrochloric Acid: HCl
• Hydrobromic Acid: HBr
• Hydroiodic Acid: HI
• Chloric Acid: HClO₂
• Perchloric: HClO₄
• Nitric Acid: HNO₃
• Sulfuric: H₂SO₄
• ELECTROLYTES

• Group 1A
• Group 2A

• strong acids
• strong bases
• soluble ionic salts

all strongelectrolytes, atrog bases, ad soluble ionic salty are siddociated into their ions when determinity the net ionic equation

solutions of an acid and a base are combined an the products are asalt an water

H and OH produces H2O

salt, carbon dioxide or sulfur dioxide, and water

• leo
• the lion says
• ger

• q is positive when system gains heat
• q is negative when system loses heat
• w is positive when work done on system
• w is negative when work done by system
• delta E positive when net gain of energy by system
• delta E negative when net loss of energy by system

• heat absorbed by the system from the surroundings
• heat released by the system into the surroundings

i.e.

• endothermic
• exothermic

6.626 x 10^-34 J-s

3.00 x 10⁸

2.18 x 10^-18 J

• n > or = 1
• l are integer ranging for 0 to n-1
• m_l are integers ranging from -l to l
• m_s have only two values: +1/2 & -1/2

• smaller
• larger

• you go down a column
• you go from right to left on a period

ions have the same number of electrons

amount of energy required to remove an electron form the ground state of a gaseous atom or ion

• you go up a column
• and left to right across a period

• opposite of ionization
• energy change accompanying the addition of an electron to a gaseous atom

you go from left to right across a row/perid

you go from left to right across a row/period and down a column

• ductile and malleable
• shiny...luster
• good conductors of electricity
• tend to form cations in aq solutions
• most metal oxides are ionic solids that are basic

• do not have luster; various colors
• solids are usually brittle, some hard some soft
• poor conductors of electricity
• nonmetal oxides are molecular substances that form acidic solutions
• tend to form anion or oxyanions in aq solutions

• ionic (electrostatic attractions b/w ions)
• covalent (sharing of electrons)
• metalllic (metal atoms bonded to several other atoms)

energy required to completely separtae a mole of a solid ionic compound into its gaseous ions

when two atoms share elecrons unequally

th ability of atoms in a molecule to attract electons to themselves

• you go from left to right across a row
• up a column

• sigma: cylindrical symmetry ofelectron density about the internuclear axis
• pi: electron density above and below the internuclear axis