Study Guide Flashcards by Anthony Sulvetta

Law

Phenomenon in nature proven to occur when certain conditions meet

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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

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Theory

(Model) is a set of tested hypothesis that gives an overall explanation of some part of nature

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Model

Activity to make something easy to understand

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Element

Substance that can’t be decomposed into simpler substances by chemical or physical means. Example: H ; Na

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Compound

Substance with constant composition that can be broken down into elements by chemical processes. Example: HNa ; PKO

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Mixture

Material of variable composition that contains two or more substances. Example: water + sugar ; the ocean

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Homogenous mixture

Mixture that is the same throughout; a solution. Example: gasoline; sugar water

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Heterogenous mixture

Mixture with different properties in different regions of the mixture. Example: jellybeans; the ocean

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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

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Chemical change

Change of substances in other substances through a reorganization of atoms; chemical reaction. Example: burning toast

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Pure substance

Substance with constant composition. Example: elements; compounds

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Calorie

Unit of measurement for energy; 1 calorie is the quantity of energy required to heat 1 g of water by 1°C

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Joule

Unit of measurement for energy. Example: 1 cal—> 4.184 joules

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Sig fig? 69678 g

5 sig figs

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Sig fig? 400607g

6 sig figs

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Sig fig? .00560g

5 sig figs

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Sig fig? 3.56 x 10^23g

3 sig figs

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Sig fig? 5600g

2 Sig figs

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Sig fig? 5600. g

4 Sig figs

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Exponential notation? .000005060 cm

5.06 x 10^-6

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Exponential notation? 5698000000 cm

5.698 x 10^9

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5.67 liters to milliliters

5.67L x 1000mL = 5670 mL

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567 Cm to m

567cm x .01m= 5.67 m

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673 degrees Celsius to kelvin

673+273= 946K

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37.6 degrees Fahrenheit to Celsius

37.6-32 / 1.80 = 3.1 Degrees Celsius

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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

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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

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Cation

Positive ion; metal forms a cation by losing electrons

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Anion

Negative ion; nonmetals form anions by gaining electrons

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Nucleus

Extremely dense; accounts for almost all of the atom’s mass; small dense of positive charge in an anion

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Electron

Negatively charged particle that occupies the space around the nucleus of an atom

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Proton

Positively charged particle

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Neutron

Particle in atomic nucleus with a mass approximately equal to that of the proton but without charge

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Na. What is the name of the element?

Sodium

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Na. What family is it in?

Group 1A

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Na. What period is in it?

Period 3

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Na. What is its atomic number?

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Na. How many protons does it have?

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Na. How many neutrons does it have?

23-11= 12

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Na. How many electrons does it have?

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Na. With what element is it isoelectronic?

Neon

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Na. Write a formula for a compound with this element and a halogen.

NaF

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Na. Write a formula for this element combined with oxygen.

Na2O

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Hydrogen acetate

HC2H3O2

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Copper (II) nitrite

Cu(NO2)2

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Nitrogen dioxide

NO2

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Phosphorus trichloride

PCl3

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Sodium phosphate

Na3PO4

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Potassium carbonate

K2CO3

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Phosphoric acid

H3PO4

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Lead (IV) chloride

PbCl4

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Tin (II) bromide

SnBr2

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Ammonium hydroxide

NH4OH

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Periodic acid

H5IO6

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Iron (II) hydroxide

FeOH2

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Carbon dioxide

CO2

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Dinitrogen pentoxide

N2O5

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Silver oxide

Ag2O

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Aluminum nitride

AlN

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Manganese (II) hydroxide

Mn(OH)2

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Ammonium carbonate

(NH4)2CO3

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Aluminum oxide

Al2O3

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Antimony pentasulfide

JbS5

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Manganese (II) oxide

MnO2

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Sulfur dioxide

SO2

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Iron (II) sulfate

FeSO4

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Hypochlorous acid

HClO

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Potassium permanganate

KMnO4

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Silver chloride

AgCl

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Copper (II) hydroxide

Cu(OH)2

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Ammonium sulfide

(NH4)2S

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Nickel (I) bromide

NiBr

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Iron (II) oxide

FeO

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Bromic acid

HBr

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Ammonium Bisulfate

NH4HSO4

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Mercury (I) sulfate

Hg2SO4

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Iron (III) oxide

Fe2O3

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Magnesium phosphate

Mg3(PO4)2

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Nickel (I) bicarbonate

NiHCO3

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Zinc hydroxide

ZnOH

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Hydriodic acid

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Diphosphorus pentoxide

P2O5

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Aluminum Phosphate

AlPO4

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Define and give examples of physical changes

Change in substances through a reorganization of atoms. Example: rust; burning toast

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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

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Define mixtures and give examples

Variable composition of pure substances. Example: water and sugar/ocean

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Define solution and give examples

Homogeneous mixture. Example: water; sugar water

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Define pure substance and give examples

Compounds/H2O And Elements/H

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What is the formula for density? What are the units of density?

D=m/v And g/mL or g/mL3

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Convert 36 mg to kg?

36,000,000

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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

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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

Sig figs? 4.00809 km

Sig figs? 6.9cg

Sig figs? .0056m

Sig figs? 6.00 x 10^3 s

Sig figs? 301.0m

Sig figs? .0039km

How many decimeters in a meter?

What is the fundamental SI unit of mass in the metric system?

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?

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

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