Study Guide Flashcards
Law
Phenomenon in nature proven to occur when certain conditions meet
Hypothesis
Propose Possible solutions to a problem or explanations for observation; suggesting such a possibility in scientific language; proposed explanation made on basis of the limited evidence at starting point
Theory
(Model) is a set of tested hypothesis that gives an overall explanation of some part of nature
Model
Activity to make something easy to understand
Element
Substance that can’t be decomposed into simpler substances by chemical or physical means. Example: H ; Na
Compound
Substance with constant composition that can be broken down into elements by chemical processes. Example: HNa ; PKO
Mixture
Material of variable composition that contains two or more substances. Example: water + sugar ; the ocean
Homogenous mixture
Mixture that is the same throughout; a solution. Example: gasoline; sugar water
Heterogenous mixture
Mixture with different properties in different regions of the mixture. Example: jellybeans; the ocean
Physical changes
A change in the form of a substance but not in its chemical nature; Chemical bonds are not broken in a physical change
Chemical change
Change of substances in other substances through a reorganization of atoms; chemical reaction. Example: burning toast
Pure substance
Substance with constant composition. Example: elements; compounds
Calorie
Unit of measurement for energy; 1 calorie is the quantity of energy required to heat 1 g of water by 1°C
Joule
Unit of measurement for energy. Example: 1 cal—> 4.184 joules
Sig fig? 69678 g
5 sig figs
Sig fig? 400607g
6 sig figs
Sig fig? .00560g
5 sig figs
Sig fig? 3.56 x 10^23g
3 sig figs
Sig fig? 5600g
2 Sig figs
Sig fig? 5600. g
4 Sig figs
Exponential notation? .000005060 cm
5.06 x 10^-6
Exponential notation? 5698000000 cm
5.698 x 10^9
5.67 liters to milliliters
5.67L x 1000mL = 5670 mL
567 Cm to m
567cm x .01m= 5.67 m
673 degrees Celsius to kelvin
673+273= 946K
37.6 degrees Fahrenheit to Celsius
37.6-32 / 1.80 = 3.1 Degrees Celsius
Given 100 g of a metal that has a volume of 63.5 mL, calculate its density. Using GESA and remember to use units
D=m/v D= 100g / 63.5 mL = 2g / mL
If the density of iron is .45 g/mL, what is the mass of a sample of metal that occupies 78 mL of volume?
.45= g/78mL —> 35g
Cation
Positive ion; metal forms a cation by losing electrons
Anion
Negative ion; nonmetals form anions by gaining electrons
Nucleus
Extremely dense; accounts for almost all of the atom’s mass; small dense of positive charge in an anion
Electron
Negatively charged particle that occupies the space around the nucleus of an atom
Proton
Positively charged particle
Neutron
Particle in atomic nucleus with a mass approximately equal to that of the proton but without charge
Na. What is the name of the element?
Sodium
Na. What family is it in?
Group 1A
Na. What period is in it?
Period 3
Na. What is its atomic number?
11
Na. How many protons does it have?
11
Na. How many neutrons does it have?
23-11= 12
Na. How many electrons does it have?
10
Na. With what element is it isoelectronic?
Neon
Na. Write a formula for a compound with this element and a halogen.
NaF
Na. Write a formula for this element combined with oxygen.
Na2O
Hydrogen acetate
HC2H3O2
Copper (II) nitrite
Cu(NO2)2
Nitrogen dioxide
NO2
Phosphorus trichloride
PCl3
Sodium phosphate
Na3PO4
Potassium carbonate
K2CO3
Phosphoric acid
H3PO4
Lead (IV) chloride
PbCl4
Tin (II) bromide
SnBr2
Ammonium hydroxide
NH4OH
Periodic acid
H5IO6
Iron (II) hydroxide
FeOH2
Carbon dioxide
CO2
Dinitrogen pentoxide
N2O5
Silver oxide
Ag2O
Aluminum nitride
AlN
Manganese (II) hydroxide
Mn(OH)2
Ammonium carbonate
(NH4)2CO3
Aluminum oxide
Al2O3
Antimony pentasulfide
JbS5
Manganese (II) oxide
MnO2
Sulfur dioxide
SO2
Iron (II) sulfate
FeSO4
Hypochlorous acid
HClO
Potassium permanganate
KMnO4
Silver chloride
AgCl
Copper (II) hydroxide
Cu(OH)2
Ammonium sulfide
(NH4)2S
Nickel (I) bromide
NiBr
Iron (II) oxide
FeO
Bromic acid
HBr
Ammonium Bisulfate
NH4HSO4
Mercury (I) sulfate
Hg2SO4
Iron (III) oxide
Fe2O3
Magnesium phosphate
Mg3(PO4)2
Nickel (I) bicarbonate
NiHCO3
Zinc hydroxide
ZnOH
Hydriodic acid
HI
Diphosphorus pentoxide
P2O5
Aluminum Phosphate
AlPO4
Define and give examples of physical changes
Change in substances through a reorganization of atoms. Example: rust; burning toast
Define and give examples of chemical changes
Change in the form of a substance, but not in the chemical nature (composition). Example: boiling; freezing water
Define mixtures and give examples
Variable composition of pure substances. Example: water and sugar/ocean
Define solution and give examples
Homogeneous mixture. Example: water; sugar water
Define pure substance and give examples
Compounds/H2O And Elements/H
What is the formula for density? What are the units of density?
D=m/v And g/mL or g/mL3
Convert 36 mg to kg?
36,000,000
How do you convert kcal to joules? Give an example.
Kcal---> joules. 1kcal ---> 4.184 joules. Convert kcals (4) to joules. 4kcals x 4.184j = 16.736j
How do you find the volume of a cube with an edge length of .10cm?
GESA Length= .10cm
V= lxwxh
V= .1x.1x.1…… Since cube all sides equal
V= .001cm^3
What are the metric prefixes for 10^6 to 10^-9?
10^6= mega 10^-9= nano
How do you convert degrees Celsius to Kelvin?
T k= C+273 C=21 K= C+273 K= 21+273 K= 294K
What is the rule of significance for adding/subtracting?
Limiting term is the 1 with the smallest number of decimal places.
Example: 23.445 + 7.830 = 31.275—> corrected —> 31.28
What is the rule of significance when multiplying/diving?
Number of significant figures in result is same as that in measurement with the smallest number of significant figures. Example: 1.342 x 5.5 = 7.381—> 7.4
Accuracy
How close you actually come to the location
Precision
Consistency in measurement
What are the rules for significant figures?
- Nonzero integers always count as significant figures. Example: 1457 has 4 significant figures
- Zeros
A. Leading zeros that precede all nonzero digits… NEVER count as significant figures. Example: .048 —> 2 significant figures
B. Captive zeros that fall between nonzero digits… ALWAYS count as significant figures. Example: 16.07 —> 4 significant figures
C. Trailing zeros are zeros at the end of the number… significant figure ONLY if contains decimal point. Example: 9.300—> 4 significant figures. Example: 150—> 2 significant figures - Exact numbers have UNLIMITED number of significant figures. Example: 1 in. —> 2.54 cm, exactly. Example: 9 pencils (obtained by counting)
Step 1 of Scientific Method
Objective
Step 2 of Scientific Method
Research
Step 3 of Scientific Method
Hypothesis
Step 4 of Scientific Method
Procedure
Step 5 of Scientific Method
Data
Step 6 of Scientific Method
Analysis
Step 7 of Scientific Method
Conclusion
Step 8 of Scientific Method
Communicate Results
What’s chemistry
Chemistry Deals with the materials of the universe and the changes that they undergo
What are two types of observations?
Qualitative. E.g: blue water
Quantitative. E.g: 591 mL
Sig figs rule for mult/div.
You’re answer can only have the same number of sig figs as your factor with the least
Sig figs when add/sub.
Answer has the same number of decimal places as the number with the least
Sig figs? 73.000g
5
Sig figs? 4.00809 km
6
Sig figs? 6.9cg
2
Sig figs? .0056m
2
Sig figs? 6.00 x 10^3 s
3
Sig figs? 301.0m
4
Sig figs? .0039km
2
How many decimeters in a meter?
10
What is the fundamental SI unit of mass in the metric system?
kg
How many mg are in 45.6g?
456
Mass formula
Density x Volume
Volume formula
Mass/density
Density formula
Mass/volume
What is the most abundant element on earth, including the crust, oceans, and atmosphere?
Oxygen
Which particle has the smallest mass?
Electron
Which Atomic particle determines the chemical behavior of an atom?
Electron
If you have 13 electrons and you lose one there are how many now?
14
If u lose an electron…
Add 1
If you gain an electron…
Lose 1
The mass number of an atom equals…
The number of protons plus the number of neutrons per atom
The number of protons in the nucleus of an atom is called…
Atomic number
What has approximately the same mass?
A proton and a neutron
In what pair does the components have the same charge?
A Neutron and a hydrogen atom
Left of staircase is
Metal
Right of staircase
Nonmetals
Where are metalloids?
In staircase
What’s the first group of metals?
Alkali metals
What is the second group of metals?
Alkaline earth metals
Middle groups?
Transition metals
Halogens are in what group?
Group 7A
What group are the noble gases in?
Group 8A
The columns are…
Groups or families
The rows are…
Periods
The elements outside of the periodic table are called…
Inner transition metals or rare earths
The State of matter for an object that has neither definite shape nor definite volume is
Gaseous
The state of matter for an object that has a definite volume but not a definite shape is
Liquid
The state of matter for an object that has both definite volume and definite shape is
Solid
Anything that has mass and volume is called
Matter
Cooking an egg
Chemical change
Boiling water
Physical change
Ironing a shirt
Physical change
Burning gasoline
Chemical change
Decomposing water
Chemical change
Evaporating alcohol
Physical change
Sanding a table top
Physical change
Grinding grain
Physical change
Fermenting fruit juice
Chemical change
Dissolving sugar in water
Physical change
“Helium is very non reactive.” Is an example of what kind of property
Chemical property
Driving a car
Chemical change
Sugar dissolving in coffee is only a ____ change
Physical
A tin can rusting is a ____ change
Chemical
Digesting a pizza is a ____ change
Chemical
In a chemical change,
Products are different substances from the starting materials
If iodine melts at 114C and boils at 184C, what is the physical state at 120*C?
Liquid
If iodine melts at 114C and boils at 184C, what is the physical state at 98*C?
Solid
If iodine melts at 114C and boils at 184C, what is the physical state at 250*C?
Gas
What describes a chemical property of gold
Good is an inert (nonreactive) metal
Burning paper is a ____ change
Chemical
Air is a ______
Pure compound
Homogenous is a ….
Mixture
Elements are on the…
Periodic table
A _____ always has the same composition
Compound
T/F. A compound can consist of one kind of element
False
An example of mixture is
The air in this room
examples of a pure substance
Elements, compounds, pure water, carbon Dioxide
T/F. Heterogenous compound
False. No such thing
Homogenous mixture=
A solution
Table salt is an example of
A compound
Chlorine gas is an example of
An element
Sand in water is an example of
Heterogenous mixture
Petroleum is an example of
Homogenous mixture
Caffeine is an example of
An element
Water is an example of
A compound
A solution can be distinguished from a compound by its
Variable composition
14k Gold
Mixture
Pure silver
Element
Aluminum
Element
Distiller water
Compound
Tap water
Mixture
Brass
Mixture
Tungsten
Element
Sodium chloride
Compound
Air
Mixture
Homogenous mixture?
Vodka
Helium is an example of
An element
The process of filtering a sand salt water mixture is a _____ process
physical
Example of What process requires chemical methods
Breaking a compound into its constituent elements
Example of What process is a chemical change
The light on a candle burns until a bell jar is placed over it for a period of time
What is an example of a homogeneous mixture
Gasoline
Diamond is a ____ state of matter
Solid
A ____ change involves a change in one or more physical properties but no change in the fundamental components that make up a substance
Physical
A ____ change involves a change in the fundamental components of the substance; a given substance changes into a different substance or substances
Chemical
Examples of Pure substances
Water, gold, ammonia
Examples of a compound
Water, ammonia
Smoke
Hetero
Air
Homo
Ocean
Hetero
River moving rapidly
Hetero
Gasoline
Homo
Mixture of 2 solids=
Alloy
Seeing difference
Hetero
Can’t see difference
Homo
Alloid
Homo
Table sugar/salt
Pure substance
Mixture = 2+ elements combined (pure substance and physical)
Example: salt and sugar combo
Vinegar and milk combo
Hetero
Elements are
Atoms and molecules… Vice versus
Density
Physical
Dissolving water
Physical
Acid on blue jeans
Chemical
NACL
Compound
Paper tearing
Physical
Rubies, emeralds
Mixtures
A match
Chemical
Rocks
Mixture
Granite
Hetero
Physical property
Phase change, directly observable, bubbling with heat (sometimes)
Chemical property
Wasn’t there before, behavior, things it’ll do, bubbling with out heat, or with (sometimes)
Exact # of sig figs
Unlimited # of sig figs
