Chemistry Semester 1 Final Review Guide – Flashcards

Chemistry is the study of matter and the changes it undergoes. Matter is the "stuff" of which the universe is composed; it as mass and it occupies space.

Physical Properties: substance shows by itself, without interacting with another substance. Chemical Properties: Properties a substance shows on interaction with other substances. Physical Change: Change that only affects physical properties. Leads to a different form of the same substance. Chemical Change: Substance (s) are changed into NEW substances.

Physical Physical Chemical Chemical Physical

exo endo

energy (heat) flows out of the system into the surroundings.

energy (heat) flows from the surroundings into the system.

atoms: the smallest particle still characterizing a chemical element elements: substance containing ONE type of atom and is defined by its ATOMIC NUMBER (# of protons in nucleus). can be bonded or "unbonded" molecules: at least two atoms (same or different) held together by bonds behaving as a unit.

An alletrope is a different molecular or crystalline form of a element. O₂/O₃, S/S₈, 3 allotropes of carbon = diamond, graphite, buckminsterfullerene.

either a pure elect or a compound.

a mixture that is the same throughout. dissolves into something.

a mixture containing regions with different properties. example: sand and water.

Substance containing only one type of atom.

Substance made by bonding atoms together in specific ways. Two or more different types of atoms.

a mixture of elements that has metallic properties.

homog compound, pure substance element, pure substance heterog compound, pure substance alloy, homog

a separation process that depends on the different boiling points of the substances.

separation of a solid from a liquid by using filter paper. Separates by size of particle.

1) a color change 2) solid/precipitate forms 3) bubbles are produced 4) flame occurs

Temperature is a measure of the kinetic energy of the particles (the faster they are going, the hotter they are). Temperature does not depend on the mass of the substance (just how many particles there are). The amount of heat energy that a substance has depends on its mass. If you double the mass, you must double the heat energy to heat it to the same temperature. The amount of heat energy that a substance has also depends on its specific heat capacity.

Thermodynamics: is the brach of physics that deals with the relationship between heat and other forms of energy. Specific Heat: among of heat per/unit mass required to raise a temperature by 1°C.

Check answer key

1 calorie = 4.184 Joules 1000 calorie = 1 kcal or Calorie

Endo = 2H₂O + HEAT → 2H₂ + O₂ Exo= 2H₂+ O₂ → 2H₂O + HEAT`

11. The energy available to do work 14. a. endothermic b.exothermic c.exothermic d.endothermic

back of old review guide problems.

Liquid water. Use the 12,500J to see how far you'll get on the heating curve. You end up at about 3°C which is LIQUID water.

251, 142 Joules

23814.2 Joules

Tin = Sn

Oxygen Hydrogen

the atomic theory 1) All elements are composed of atoms 2) All atoms of a given element are identical. 3) Atoms of different elements differ. 4) Compounds consist of different elements. 5) Atoms are not created nor destroyed in a chemical reaction.

electrons reside in distinct energy levels

developed five principles from the three atomic laws

gold foil experiment proved existence of a positive core

plum pudding model featuring neg. charged. electrons in a ball of pos. charge.

Mole

P=E (usually) Mass - P = N

²³⁴U ²³⁸ U

Groups- down (columns) Periods - across (rows)

DRAW ON PERIODIC TABLE

1 Molecule 6 Carbon, 12 Hydrogen, 6 Oxygen

charge and group number.

Alpha, Beta, Gamma Gamma is most penetrating.

a. alpha particle ⁴He b. missing particle is ¹⁵N

It is a 'salt' consisting of only two elements in which both elements are ions, one anion and one cation.

H₂O, Ch₄, So₂, FeO

look at polyatomic chart, and back of old review guide.

ate → ic ite → ous Use hydro for binary acids aka. H₂Se

atom is neutral (number of protons = electrons) Ions are charged (protons DO NOT equal number of electrons). Cation = positive

SnCl₂

Iron (III) Oxide

Fe(NO₃)₃

Magnesium Sulfate Heptahydrate

Al(OH)₃

Barium Chlorate

Copper Phosphate

mono, di, tri, tetra, hexa, hepta, octa, nona, deca

mass per unit volume

2.70 g/mL

1 g/mL

look at pink chart and book. know conversion factors.

K m s

4.021m

470,000 cg

2.9 x 10 ⁻⁸ sec

62 Km

4,5,3,1

left positive exponent. right negative exponent.

amount of a certain substance

6.022 x 10 ²³

chemical formula

avagadros #

molar mass

940.0 moles Xe

2.0 X 10²⁴ atoms

5.04 X 10⁻³ moles Cu

212 g

3.19 X10⁻⁸ g

80.0 g

0.72 moles

mm= 331.2 g/mol percent composition: 62.6% Pb 8.46% N 29.0% O

mm= 74.1 g/mol percent composition: 54.1% Ca 43.2 % O 2.71 % H

HgSO₄

CH

C₆H₆

to provide energy needed to break bonds and bring atoms close enough to react.

Mg (s) + 2H₂O(l) → Mg(OH)₂ + H₂ (g)

Fe₂O₃ +2Al(s) → 2 Fe(s) + Al₂O₃

2KClO₃ (s) → 2KCl + 3O₂ (g)

C₉H₂0 + 14O₂ → 9O₂+ 10 H₂O