exam 1 Flashcards by Aubrey Pennington

the branch of science that deals with the identification of the substances of which they interact, combine, and change; and the use of these processes to form new substances

definition of chemistry

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anything that occupies space

matter

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it is a list of physical and chemistry aspects

properties

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has a definite (constant) composition and distant properties

substance

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of or relating to chemistry or a substance with a distinct properties that is produced by or used in a chemical process

chemical

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examples of chemicals

H2O
CO2
ethanol

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a method of procedure that has characterized natural science since the 17th century, consisting in systemic observation, measurement, and experiment, and the formulation, testing, and modification of hypothesis

scientific method

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a supposition or proposed explanation made on the basis of limited evidence as a starting point for further investigation

hypothesis

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an experiment is an orderly procedure carried out with the goal of verifying, refuting, or establishing the validity of a hypothesis

scientific experiment

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is a well substantiated explanation of some aspects of the natural world, based on knowledge that has been repeatedly confirmed through observation and experimentation

scientific theory

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statement based on repeated experimental observations that describes some aspect of the world

scientific law

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2 or more atoms attached together in a specific geometrical arrangement, these attachments are called bonds

molecules

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are attractive forces that hold atoms together

bonds

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basic unit of a chemical element

atom

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the rearrangements of atoms to form new substances

chemical reaction

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mass neither created nor destroyed in chemical reactions so we use coefficients to balance the mass

law of conversion of mass

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aluminum

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argon

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barium

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boron

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Bromine

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calcium

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carbon

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arsenic

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cadmium

francium

strontium

krypton

arsenic

chlorine

fluorine

Helium

Hydrogen

iodine

lithium

magnesium

beryllium

cobalt

neon

cesium

xeon

manganese

nitrogen

oxygen

Phosphorus

Silicon

sulfur

zinc

uranium

chromium

nickel

platinum

radon

copper

iron

lead

mercury

potassium

silver

sodium

gold

tin

titanium

antimony

tin

can not be separated by physical means

pure substance

can not be chemically broken down into simpler substances (make up everything)

element

combination of two or more elements (different)

compound

can be separated by physical means (combination of substances)

mixture

composition of the mixture is uniform throughout

homogeneous mixture

composition is not uniform

heterogeneous mixture

most common type of fatal air poisoning in many countries

carbon monoxide

third most common gas in the atmosphere

carbon monoxide

what is the capacity to do work

energy

push or pull on an object

force

energy of motion

kinetic energy

form of kinetic energy because it is caused by molecular motion

thermal energy (heat)

(J) the amount of energy needed to raise the temperature of one gram of water

joule

1 calorie equals how many joules

4.184

to have a successful reaction you need

- a collision - enough energy - the right orientation

reactions that absorb heat

endothermic reactions

reactions that release heat

exothermic reactions

stored in the bonds

potential energy

energy released or absorbed in the chemical reaction

kinetic energy

the "absolute temperature scale" begins at absolute zero and only has positive values

kelvin

the temp scale used by science, formally called centigrade, most commonly used scale around the world, water freezes at 0* C and boils at 100*C

celsius

commonly used scale in the US for our weather reports; water freezes at 32*F and boils at 212*F

Fahrenheit

things you can count or defined equalities things like 1000mg= 1g or you count 5 coins

exact numbers

numbers that come from a device that measures things like height, weight, temp

measured numbers

expressed using numbers (trying to be exact as possible)

quantitative

expressed using properties (using senses or making general observations)

qualitative

the closeness of the set of values

precision

closeness of a single measurements to its true value

accuracy

Rule #1 for Sig Figs

all non zero digits are significant

Rule #2 for Sig Figs

interior zeros are significant

Rule #3 for Sig Figs

leading zeros are NOT significant

Rule #4 for Sig Figs

trailing zeros count if there is a decimal point

Rule #5 for Sig Figs

trailing zeros may or may not be significant

smallest unit of matter that has the characteristics properties of a chemical element

atom

atoms contain subatomic particles

- protons - electrons - neutrons

what charge do protons have

positive

what charge do electrons have

negative

where does most of the size of an atom come from

the cloud around the nucleus

where is most of the mass contained

in the nucleus

what is the protons AMU

1.007

where is the proton located

nucleus

what is the neutrons AMU

1.008

where is the neutron located

nucleus

what is the electrons AMU

0.00055

where is the electron located

outside the nucleus

an atom or molecule with a net electric charge due to the loss or gain of one or more electrons

ions

positive ions are called

cations

negative ions are called

anions

what do metals always form

positively charged cations

what do nonmetals normally form

negatively charged anions

two or more forms of the same element that contain equal numbers of protons but different numbers of neutrons

isotopes

what are isotopes identified by

mass number

when the elements are arranged in order of increasing atomic mass, certain sets of properties periodically

periodic law

- solids at room temp, except Hg - shiny - conduct heat - conduct electricity - malleable - ductile - lost electrons and form cations in reactions - lower left on the table

metals

- poor conductors of heat - poor conductors of electricity - solids are brittle - gain electrons in reactions to become anions - upper right on the table - except H

nonmetals

show some properties of metals and some of nonmetals

metalloids

the weighted average of all the naturally occurring isotopes for that element

atomic mass

when electrons have been transferred between atoms, resulting in oppositely charged ions that attract each other and have a net charge of zero

ionic bonds

result when two atoms share some of their electrons

covalent bonds

elements whose particles are single atoms

atomic elements

elements whose particles are multi atom molecules

molecular element

compounds whose particles are molecules made of only nonmetals

molecular compounds

compounds whose particles are cations and anions this is normally a compound composed of a metal with a nonmetal

ionic compounds