Definitions

Question 1

Kelvin

Answer 1

K= c*+ 273
That means that when kelvin is at 273 Celsius is 0
0 Kelvin is Absolute Zero ( lowest temp in universe)
Kelvin scale absolute temperature
Fahrenheit is different

Question 2

Intensive Property

Answer 2

Does NOT depend on amount (color,boiling point,freezing point, density)

Question 3

Law of Conservation of Energy

Answer 3

Energy can not be destroyed, only changed into another

Question 4

Law of definite Proportions

Answer 4

(1/2=50%, 1/2=50%) same proportion by mass

Question 5

Substance

Answer 5

Matter which all samples have identical composition and proprties

Question 6

Measurements in Chemistry

Answer 6

Length=meter (m),
mass= kilograms(Kg) , time=seconds(S) ,
Current=Ampere(A) , Temperature= kelvin(K) ,
Amount of substance=Mole(mol)

Question 7

Weight

Answer 7

Measurement of the gravitational attraction for a body

Question 8

Mass

Answer 8

Measurement of the quantity of matter in a body

Question 9

Energy

Answer 9

Capacity to do work or transfer heat

Two types: potential energy and kinetic energy

Question 10

1 meter

Answer 10

39.37 inches

Or 3.28 ft

Question 11

Conversion factors of Length

Answer 11

1 inch = 2.54 cm
1 meter = 39.37 inches
1 meter = 3.28 ft
1 mile = 1.60 Km

Question 12

Conversion factors of Volume

Answer 12

1gallon= 3.785 liters
1 gallon= 4 quarts
1 gallon= 2 pints
1 quart = 0.946 liters
1 pint = 0.473 liters

Question 13

Conversion factors of Mass

Answer 13

1 pound = 453.6 g
1 Kg = 2.204 lb
1 oz= 28.34 g

Question 14

Accuracy

Answer 14

How closely measured values agree with the correct value

Depends on operators skill and calibration of instrument

Question 15

Precission

Answer 15

How closely individual measurements agree with each other
Depends on instrument quality and sensitivity
Precision precedes accuracy

Question 16

Density

Answer 16

Density = mass (g)
_________
volume (ml)
D= m/ v. Or m= D x V. Or V= m/D

Question 17

Significant figure rules

Answer 17

Leading zeroes are never significant
All non zeroes are significant
Zeroes at the end( trailing) are significant if they are preceded by a decimal point
Imbedded zeroes are significant

Question 18

Fahrenheit

Answer 18

F= 9/5(c) + 32

Or F= (1.8 x c) +32

Question 19

Specific Gravity

Answer 19

Same as Density, but without the symbols
              Ex  D= 11.4 g/ ml  , specific grav= 11.4
Density substitute (g/ml)
\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_
density of water (1.00 g/ml)

Question 20

Specific heat (s)

Answer 20

Amount of heat or energy necessary to raise the temperature of 1 gram of a substance by 1c*
q=m x s x ^t. Or s=q/m x ^ t –equation to finding specific heat
s= cal/ g x c. Or s= joule/ g x c– specific heat units
[q is heat energy in calories or joules, m is mass grams, s is specific heat cal or joules/ g x c*, ^ t is temp change ( initial-final temp)]

Question 21

Units of Heat

Answer 21

Joule (si unit)and Calorie

1 calorie=4.184 joules

Question 22

Calirometry

Answer 22

Measurement of heat changes
Exothermic process
Or endothermic process= absorption of heat

Question 23

Heat

Answer 23

Total sum of Energy, kinetic + potential

Is extensive quantity, the more mass the more heat

Question 24

Calorie

Answer 24

Heat or energy required to raise the temperature of 1 gram of WATER by 1 c*
Kilocalorie ,Kcal, is 1000 cal is 1 nutritional calorie

Question 25

Atom

Answer 25

Smallest particle of an element that keeps its identity, stays the same through physical and chemical changes.

Question 26

Molecule

Answer 26

Smallest part of an element that can have a stable independent existence in nature. H2, O2, S2, H2O, CH4, C2H5OH

Question 27

Homogeneous mixture

Answer 27

The same throughout, no physical boundaries and it doe not separate. Air, milk, alloys, alcohol...

Question 28

Heterogeneous mixtue

Answer 28

Mixtures are not the same throughout and posses boundaries | Sand, concrete, ...

Question 29

Metals

Answer 29

Good conductors of electricity and heat, shiny, ate monoatomic. Alkali Alkali earth Transition

Question 30

Non metals

Answer 30

Monoatomic, diatomic, or polyatomic Diatomic. H2,N2 , O2,; halogens F2 ,Cl2 ,Br2 ,I2 . Polyatomic: P4 ,S8; C60 ,C70

Question 31

Ionic compounds

Answer 31

Metal and non metal, contain electric charge, Change in anion must be the same as cation Cations positively charged-ions, less than neutral Anions negatively charged ions, more than neutral Cations go in front of anions

Question 32

Famous Ions

Answer 32

``` Cations: Na+, Ca +2, Al +3, NH4+ Ammonium Anions -1: Cl-,CN- Cyanide, SCN-Thiocyanate, MnO4-Permanganate OH- Hydroxide,C2H3O2-Acetate -2: SO4-2Sulfate, O2-2Peroxide, C2O4-2Oxalate, CrO4-2Chromate,Cr2O7-2Dichromate -3: CPO4-3 , ```

Question 33

Atomic Theory of Matter

Answer 33

Atoms are the building blocks of matter Atoms of the same elements are identical physically and chemically Atoms are neither created nor destroyed in chemical reactions In chemical reactions they are rearranged united or separated to produce new substances Atoms combined in a fixed proportion by weight to produce homoatomic molecules or heteroatomic molecules(compounds)

Question 34

Formulas of ionic compounds

Answer 34

NaCl Sodium Chloride Na+ ,Cl- KOH Potassium Hydroxide K+,OH- CaSO4 Calcium Sulfate Ca+2,SO4-2 Al(COH)3 Aluminum Hydroxide Al+3 ,3OH-

Question 35

More Ionic Compounds

Answer 35

H2SO4 Sulfuric Acid. FeBr2 Iron(II) bromide C2H5OH Ethanol. HNO3 Nitric Acid SO3 sulfur trioxide. FeBr3 Iron Bromide or Iron(III) Bromide K2SO3 Potassium Sulfite---K2- , SO3-2

Question 36

Atomic mass Diameter

Answer 36

1 x 10 -10 m

Question 37

Rutheford

Answer 37

Atom is mostly open space Nucleus is small dense center Nucleus has most of the mass Mass. 1/100,000

Question 38

AMU

Answer 38

Atomic mass unit= atomic weight= found in the periodic table expressed in amu or amu/ atom Is also the Relative Mass = the average of an element's isotopes found in nature with their relative abundance.

Question 39

Homoatomic molecules

Answer 39

Molecules made of the same element Diatomic or polyatomic O2,H2 ,C60

Question 40

Atomic mass diameter

Answer 40

1x 10-10 meters approximately Ex how many atoms in 1 .00 mm 1.00 mm. X 1 x 10-3 m. X 1 atom __________. ________ 1.00mm. 1 x10-10 m

Question 41

Atomic mass

Answer 41

1 x 10-23g. Ex. 1.00 mg x 10-3 g. X. 1atom __________. _______. ______ atom. 1 mg. 1 x10-23 g

Question 42

Some chemical properties of metals

Answer 42

Outer shells contain few electrons Form cations by loosing electrons Form ionic compounds with nonmetals Solid state characterized by metallic bonding

Question 43

Some properties of non metals

Answer 43

Outer shells contain four or more electrons Form anions by gaining electrons Form ionic comp with metals and covalent comp with other non metals Noble gasses are part of non metals

Question 44

Nuclear density

Answer 44

15 10. g _________ mL

Question 45

James Chadwick

Answer 45

1932 discovered Neutrons

Question 46

H.Gj Moseley

Answer 46

1913 said atomic # determines element | All elements differ by atomic #

Question 47

Mole

Answer 47

Number of atoms, ions or molecules Like a dozen = 12 of something 23 One Mole = 6.022.x 10. -Avogadro's number

Question 48

Molar Mass (MM)

Answer 48

Molar Mass in grams of an atom=to atomic weight in amu (atomic mass units) from periodic table of an element--g Ex. Atomic weight of H is 1.00794 is expressed in g/mol or amu/atom

Question 49

How to find # of Moles

Answer 49

Avogadros#.- from atoms to moles is one step -from grams to moles. Is one step - from atoms to grams. Are two steps Atoms x Moles x grams. Or grams x Moles x atoms 1 mole of an element / 6.022 x 10 to23. --- grams(atw)of an element/1mole Ex. Mg atom to gram-- 1 Mg atom X 1 mol Mg atom X 24.30g Mg ------------------ ----------- =4.04x10to23gMg 6.022x10to23Mg atoms. 1mol Mg atoms