Chemistry Midterm

Chemistry with Addabo at Immaculate Heart Academy

About this deck

By: McKenna Blake
Created: 2011-01-17
Size: 128 flashcards
Views: 157

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Law of conservation of Mass

matter is neither created nor destroyed during ordinary chemical or physical changes.

Law of Definite proportions

a chemical compound contains elements in exactly the same proportions by mass

Law of Multiple Proportions

if 2 or more compounds are composed of the same element, then the ratio of the masses of the second element combined with the certain mass of the first element always a ration of small whole numbers.

Dalton's atomic theory

1. All matter made up of tiny particles called atoms.

2. Atoms of a given element are alike in size, mass, and properties. Atoms of different elements are different in size, mass and properties.

3. Atoms cannot be created, subdivided or destroyed.

4. Atoms of different elements ‘combine in simple whole number ratios, forming compounds.

5. Atoms are combined, separated, or rearranged in chemical reactions.

Democritus

invented the atom

Dalton

published his atomic theory in 1808

Thomson

discovered the electron and its charge to mass ratio using cathode ray experiment.

Millikan

measured the charge of the electron and calculated its mass using an oil drop experiment .

Rutherford

discovered the nucleus of the atom using the Gold foil experiment.

Chadwick

discovered the neutron

Thomson’s cathode ray

- Made up of a stream of electrons

- Glow is caused by a stream of negatively charged particles

- Led to the discovery of the electron

- Cathode and Anode on each side

Rutherford's Gold Foil experiment

- discovery of the nucleus

- most alpha particles passed through the Au foil with little to no deflection

- positive charge of the atom is not diffused but concentrated in the nucleus.

-atoms were mostly empty space

Atomic Mass Unit

a unit of mass that is exactly 1/12 the mass of a carbon- 12 atom

Nuclear forces

short- ranged forces that hold the nuclear particles together.

Proton

positively charged/nucleus/mass- 1

Neutrons

electrically neutral/ nucleus/ mass- 1 (slightly more than proton)

Electron

negatively charged/ electron cloud/ mass 0 (1/2000)

Nuclide

a general term for any isotope of any element.

Mass number

the total number of protons and neutrons in the nucleus.

Atomic number

the number of protons in the nucleus of an atom of that element.

Mole

the amount of a substance that contains as many particles as there are atoms in exactly 12 grams of carbon -12.

Avogadro's number

6.022 x 10 ²³

formula unit

simplest collection of atoms from which an ionic compound's formula can establish

formula mass

sum of the masses of all the atoms in a formula.

percent composition

percent by mass of each element in a compound

molar mass

the mass of one mole of a pure substance

average atomic mass

the weighted average of the atomic masses of the naturally occurring isotopes of an element.

Chemistry

the study of the composition, structure, and properties of matter and changes it undergoes.

Organic chemistry

the study of most carbon- containing compounds

Inorganic chemistry

the study of all substances not classified as organic, mainly the compounds that do not contain carbon.

Physical chemistry

the study of properties and changes of matter and their relation to energy

Analytical chemistry

the identification of the components and composition of materials.

Biochemistry

the study of substances and processes occurring in living things.

Theoretical chemistry

the use of mathematic and computers to understand the principles behind observation observed chemical behavior and to design and predict the properties of new compounds.

six branches of chemistry

Organic, inorganic, physical, analytical, biochemistry and theoretical

Basic research

increases knowledge (chance discoveries)

Applied research

solves a problem

Technologic development

involves the production and use of products that improve our quality of life.

Matter

anything that has a mass and takes up space.

Properties

characteristics that can be used to identify or classify substances.

Malleable

can be pounded into sheets

Ductile

drawn into wire

Luster

shine

Inertia

tendency of an object to resist chance in motion

Chemical

any substance that has a definite composition.

Physical change

a change in a substance that does not involve a change in the identity of the substance

i. Grinding, cutting, melting, and boiling

Chemical change

a change in which one or more substance(s) is converted into different substance(s).

Reactants

substances that react in a chemical change.

Products

substances that are formed by chemical changes.

Extensive properties

depends on the amount of matter that is present.

i. Volume, mass, amount of energy

Intensive properties

do not depend on the amount of matter

i. Melting point, boiling point, density, ability to conduct electricity and heat

Solid

defined volume and shape/ no compressibility. held close to each other and vibrates

Liquid

indefinite shape and definite volume/ no compressibility. Particles flow and glide closely together.

Gas

indefinite shape and indefinite volume/ very high compressibility. Freely and more far apart

Plasma

a high temperature physical state of matter in which atoms lose their electrons.

Mixtures

a blend of two or more kinds of matter, each of which retain its own identity and properties.

Homogeneous

uniform in composition

Also called solutions

Particles

do not settle down, cannot be filtered out and too small to shatter light

Heterogeneous

uniform throughout

Colloids

1-100 (fog) light can pass through

Suspension

greater than 1-100^th, large enough to scatter light.

Pure substanse

substance that has a fixed composition and differs from a mixture in that every sample of a given pure substance has exactly the same characteric properties and composition.

Element

a pure substance made of only one kind of atom.

mass

measurement of the amount of matter

matter

anything that has mass and takes up space

atom

the smallest unit of an element that maintains the properties of that element

compound

a substance that is made from the atoms of two or more elements that are chemically bonded

molecule

smallest unit of an element or compound that retains all of the properties of that element or compound

volume

amount of space an object occupies

scanning electron microscope

reveals tiny structures by beaming particles called electrons at materials

Non metals

a. to the right of the staircase/poor conductor of electricity

i. gases including hydrogen, oxygen, chlorine, fluorine and noble gases.

Solids include carbon, sulfur, iodine, selenium and phosphorus

Metalloid

a substance with some characteristics of metals and some characteristics of nonmetals

metal

type of element that is a good conduct of electricity

group/families

elements in the vertical columns in the periodic table

periods

the horizontal rows of elements in the periodic table

noble gases

the elements in group 18 of the periodic table that are nonreactive

quantity

something that has magnitude, size or amount

theory

a generalization that explains a body of known facts or phenomena.

Mass SI base unit

Kilograms- kg

(anything with grams)

Time SI base unit

seconds- s

volume SI base unit

cubic meters- m³

Length SI base unit

meter- m

(anything with m or L)

Temperature

kelvin (K)

Density

kilogram per cubic meter- Kg/m3

(anything with a fraction)

weight

a measure of the gravitational pull on matter

Area Derived SI Units

square meter- m²

volume

the amount of space occupied by an object

Density

the ratio of mass to volume, or mass divided by volume.

kilogram symbol

mole symbol

mol

centi

0.01

10 ^-2

micro

u (backwards)

0.000 001

10 ^-6

deci

0.1

10^-1

milli

0.001

10 ^-3

nano

0.000 000 001

10 ^-9

pico

0. 000 000 000 001

10 ^-12

Transform a statement of equality to a conversion factor:

Quality sought= quality given * conversion factor

Accuracy

close a measurement is to an accepted value

Precision

reproducibility of a series of measurements.

Percent Error

accepted value - experimental value

--------------------------------------------------------------- x 100

Accepted Value

all nonzero digits are ...

always significant

captive zeros (zeros between non zero digits) are ...

always significant

leading zeros ( to the left of non zero digits) are...

never significant

ex. 0.75 or 0.0023

trailing zeros (to the right of the nonzero digits) are..

sometimes significant

Significant if there's a decimal point in the number

ex. 53, 000.0

Addition or subtraction with significant figures

should have the same number of decimal places as the measurement with the fewest decimal places.

multiplication and division with significant figures

should have the same number of significant figures as the measurement with the fewest decimal places.

Rounding greater than 5

increases by 1

Rounding less than 5

stays the same

Rounding 5, followed by nonzero digits

increases by 1

Rounding 5 not followed by nonzero digits and preceded by an odd digit

increases by 1

Rounding not followed by nonzero digits and the preceding significant digits is even

stays the same

Direct proportion

straight line

inverse proportion

curved line

qualitative

date that describes info

- shape, color, odor

quantitative

numerical info

- mass, volume, boil, melt

hypothesis

a testable statement used for making predictions and carrying out further experiments

control

basis for comparison in an experiment

independent variable

adjusted by the experiment

variables

factors that change

dependent variable

changes due to independent variables

constant

stays the same

About this deck

By: McKenna Blake
Created: 2011-01-17
Size: 128 flashcards
Views: 157

About StudyBlue

“I have used this website for three exams, and I see a huge difference in my test results.”
Naj