chemistry--ch.1

science

place of naturalism and materialism

matter

anything that takes up space and has mass (that weighs something)

pure substances and mixtures

two types of matter?

pure substances

elements or compounds

mixtures

homogeneous or heterogeneous

pure substance

made up of only ONE type of substance; one chemical formula or symbol

element

SIMPLEST type of matter; made up of only one type of atom

ex) Nitrogen, Oxygen…

atom

smallest unit of matter; keeps it unique characteristics

compound

pure substance made of TWO OR MORE elements chemically joined together

mixture

combination of two or more substances; can be separated into its different components

homogeneous mixture

one whose composition is the SAME throughout

heterogeneous mixture

one whose composition is NOT UNIFORM but VARIES throughout

periodic table of the elements

listing of all the elements on earth; each block holds a different element, has a letter or two, have numbers above and below these letters

chemical symbol

letters on the periodic table; ex) Na = sodium, Au = gold

group

vertical column; have SIMILAR chemical behaviors; A designations for main-group elements, B designations for transition elements

IUPAC (International Union of Pure and Applied Chemistry)

system using numbers 1 through 18 for the columns

period

horizontal row on periodic table; numbered from 1 to 7; staircase-shaped line which begins at boron, separates metals from nonmetals; elements bordered by the line, with the exception of aluminum (Al) are metalloids

largest quantity

how much do you need the elements of carbon (C), hydrogen (H), oxygen (O), and nitrogen (N)

macronutrients

needed in quantities greater than 100 mg per day; ex) Sodium (Na), magnesium (Mg), potassium (K), calcium (Ca), and chlorine (Cl)

micronutrients

needed in quantities less than 100 mg per day; ex) Iodine (I), fluorine (F), iron (Fe), zinc (Zn)…

hydrogen, carbon, nitrogen and oxygen

most common elements in living things?

chemical formula

identifies which elements and how many atoms of each element are present in a compound; ex) H2O or NaCl

gas

state of matter composed of particles that are not associated with each other and are rapidly moving, NO definite volume or shape

liquid

state of matter composed of particles that are loosely associated and freely moving, DEFINITE volume but NO definite shape

solid

state of matter composed of particles that have an orderly arrangement and very little motion, DEFINITE shape and DEFINITE volume

physical change

change in the STATE; form of the matter is changed, but not its identity

chemical change

change in the chemical identity of a substance; substance undergoes such a change it is a chemical reaction

chemical reaction

change in the chemical identity of a substance

reactants and products

2 terms in what happens in a chemical reaction?

law of conservation of mass

mass either created or destroyed; number of atoms of each element in the reactants equals the number of atoms of each element in the products (number of atoms must be the same on BOTH SIDES of the equation = balanced)

matter only changes form

coefficients

numbers in front of the chemical formula in order to balance a chemical equation

systeme international d’Unites (SI)

modern-day version of the metric system

kilogram (kg)

SI unit for mass

liter (L)

SI unit for volume

meter (m)

SI unit for length

giga

x 1,000,000,000

mega

x 1,000,000

kilo

x 1,000

base unit

1 (gram, liter, meter)

deci

divided by 10

centi

divided by 100

milli

divided by 1000

micro

divided by 1,000,000

nano

divided by 1,000,000,000

equivalent units

quantities that can be related to each other by an equal sign; 1 dL = 0.1 L

conversion factors

equivalencies that can be used to convert one unit to another using one or more of these factors

dimensional analysis

use of converting units to an equivalent unit

significant figures

all digits in a number representing data or results that are known with certainty plus one uncertain digit

measuring matters; important to be reasonably; nondigital device, there is some level of uncertainty in the measurement; the sig figs are the digits with certainty plus one estimated digit; digital devices automatically show us the number of sig figs; all NONZERO numbers are considered significant

C

unit for coefficient

n

exponent telling us the number of tens places that apply

scientific notation

C x 10^n

positive

? exponent that tells us that the actual number is greater than 1

negative

? exponent tells us that the number is between 0 and 1

sig figs

in scientific notation, only ? ? are shown in the coefficient

percent

%; part out of 100 total, or hundredths; directly compare two sets of numbers that have different total sizes

% = part/whole x 100

mass

measure of the amount

gram (g)

common unit for mass

pull of gravity

weight is determined by ? ? ? on the object; force changes depending on location

volume

measure of the SPACE occupied by matter

milliliter (mL)

SI unit used for volume in the lab

cubic centimeter

unit used in the clinical setting for volume; 1 mL = 1 cc or cm³

density (d)

ratio of mass (m) to its volume (V)

d = m/V

constant at a given temperature

specific gravity (spgr)

ratio of the density of a sample to the density of water

= density of sample/density of water

refractometer

measures the specific gravity of a liquid

temperature

measures the hotness or coldness; SI unit for temperature = Kelvin

measure also by Fahrenheit and Celsius

hyperthermia

person’s temperature is ABOVE 40.0 deg C (104 deg F)

cause convulsion, coma, or permanent brain damage

hypothermia

person’s temperature DROPS BELOW 35 deg C (95 deg F)

feels cold, has an irregular heartbeat, and slow breathing rate

energy

capacity to do work or supply heat

potential energy

stored energy

kinetic energy

energy of motion

law of conservation of energy

energy takes various forms, but it is never created or destroyed

joule (J)

SI unit for energy

calorie

amount of energy required to raise the temperature of ONE gram of water by one degree Celsius; 1 calorie = 4.184 joules

Calorie (Cal)

1000 times larger than a calorie; 1 Calorie = 1000 calories

heat

kinetic energy; flows from a warmer body to a colder one

every substance has the ability to absorb or lose this as the temperature changes

specific heat capacity

amount of heat NEEDED to raise the temperature of 1 g of that substance by 1 deg C

SH = heat/grams x delta T

metals

low specific heat values

water

very high specific heat; 1.00

state of matter

physical form in which the matter exists; most common are solid, liquid, and gas

accuracy

degree of agreement between the true value and the measured value

error

difference between the true value and our estimation

can be random or systematic

precision

measure of the agreement of REPLICATE measurements

deviation

amount of VARIATION present in a set of replicate measurements

12 in

1 ft =

5280 ft

1 mile =

16 oz

1 lb =

drop factor

used to determine drip rates when a prescribed volume of medicine is required in a given time period

drop

gtt means…