Chemistry Midterm

scientific notation

used when writing very large or very small numbers, expresses a number as a product of a number between 1 and 10 and the appropriate power of 10

english system, metric system, international (SI) system

three unit systems

kilogram (kg)

SI unit for mass

meter (m)

SI unit for length

second (s)

SI unit for time

kelvin (K)

SI unit for temperature

liter (L)

SI unit for volume

accuracy

how close your average answer is to the correct answer

precision

the ability to reproduce results in the lab

not accurate, precise

this picture is showing

not accurate, not precise

this picture is showing

accurate, not precise

this picture is showing

accurate, precise

this picture is showing

(| accepted - experimental |) / accepted

formula for finding % error

5

less than \___% error is accurate

measurement

always has some degree of uncertainty, should include all certain numbers plus one estimated number

significant figures

all of the numbers recorded in a measurement

certain, estimated

significant figures include all of the \___ numbers and one \___ number

significant

all numbers that are not zeros are \___

significant

all sandwiched zeros are \___

significant

all ending zeros following a decimal are \___

not significant

all leading zeros are \___

left, right, zeros, non-zero

To find the number of significant figures if a decimal is present in a number, you read from \___ to \___, skip any \___, and count from the first \___ number to the end

right, left, zeros, non-zero

To find the number of significant figures if a decimal is absent, you read from \___ to \___, skip any \___, and count from the first \___ number to the end

3

10.0 has \___ sig fig(s)

1

0.0004 has \___ sig fig(s)

1

100 has \___ sig fig(s)

4

101900 has \___ sig fig(s)

infinite

12 eggs has \___ sig fig(s)

least

In multiplication and division, the answer should have the same number of sig figs as the number in the problem with the \___ number of sig figs

greatest smallest, smallest

In addition and subtraction, the answer should be rounded to the same last numerical place as the number in the problem with the \___ \___ numerical place (usually with the \___ number of decimals)

100, defined value, infinite

In the formula for percent error, the \___ that is multiplied is not accounted for when trying to find sig figs because it is a \___ \___ and has an \___ number of sig figs

10^3

the prefix kilo is \___ times the base

kilo

the prefix \___ is 10^3 times the base

10^6

the prefix mega is \___ times the base

mega

the prefix \___ is 10^6 times the base

10^-1

the prefix deci is \___ times the base

deci

the prefix \___ is 10^-1 times the base

10^-2

the prefix centi is \___ times the base

centi

the prefix \___ is 10^-2 times the base

10^-3

the prefix milli is \___ times the base

milli

the prefix \___ is 10^-3 times the base

10^-6

the prefix macro is \___ times the base

macro

the prefix \___ is 10^-6 times the base

10^-9

the prefix nano is \___ times the base

nano

the prefix \___ is 10^-9 times the base

mL

1 cm^3 \= 1 \___

cm^3

1 mL \= 1 \___

L

1 dm^3 \= 1 \___

dm^3

1 L \= 1 \___

defined values, infinite

equivalency statements are \___ \___ and therefore have an \___ number of sig figs

factor label method

a method of using ratios to covert from one unit to another

numerator, denominator

you can change the power of any conversion factor as long as you do it to both the \___ and \___

density

a numerical value that represents the ratio of mass to volume for a given substance

M/V

D\=\___

DV

M\=\___

M/D

V\=\___

water displacement method

to calculate volume of irregularly shaped objects, the \___ is used

mass

In a density graph, the Y axis \= \___

volume

In a density graph, the X axis \= \___

density

In a density graph, the slope \= \___

0

In a density graph, the Y intercept \= \___

rise/run \= mass/volume \= density

equation to find density

mass, volume

In molecular drawings for density, the size or number of particles represents \___ while the size of the container represents \___

physical properties and changes

the matter does not make new or break old chemical bonds

chemical properties and changes

the matter does make new or break old chemical bonds

physical change

ripping is an example of a \___

physical change

bending is an example of a \___

physical changes

phase changes are examples of \___

physical change

dissolving is an example of a \___

chemical change

color change is an example of a \___

chemical change

precipitate formation is an example of a \___

chemical change

gas release (bubbling or fizzing) is an example of a \___

chemical change

heat release or absorption is an example of a \___

chemical change

a lack of a reaction indicates a \___

intrinsic property

a property that is independent of how much of the material is present

extrinsic property

a property that is dependent on the amount of material present

intrinsic properties

density and color are examples of \___

extrinsic properties

mass and volume are examples of \___

solid

the state of matter that is rigid, a fixed shape and volume, have little atomic motion, and are high in density

solid

this picture is showing a \___

liquid

the state of matter that is fluid, has a definite volume but takes that shape of its container, has some atomic motion, and has medium density

liquid

this picture is showing a \___

gas

the state of matter that has very unique properties, is compressible, has low density, expands, has no definite shape and volume, and has high atomic motion

gas

this picture is showing a \___

heating/cooling, pressure change

two ways to change the state of matter

physical

changing the state of matter is a \___ change

matter

anything that has mass and takes up space

pure substances, mixtures

two types of matter

physically, chemically

mixtures are \___ combined, not \___ combines

pure substance

a substance that is made up of one kind of matter

uniform, constant

pure substance are \___ and have \___ properties

elements and compounds

two types of pure substances

element

the simplest form of matter that is made of atoms or molecules, can not be broken down, and is identified by number of protons

compound

a chemical combination of two or more different elements that is made of molecules or formula units (ionic compounds), can only be separated with chemical processes, have unique properties when compared to the elements that make up them, and have defined ratios of atoms

mixture

any sample of matter that is made up of at least two different substances, the parts are not chemically combined, and can be separated with physical processes

homogeneous, heterogeneous

two main types of mixtures

heterogeneous mixture

a mixture that does not look uniform throughout

suspension, colloid

two types of heterogeneous mixtures

suspension

a heterogeneous mixture that has two distinct layers