chemistry final

Chemistry

the science that deals with the materials of the universe and the changes that theres materials undergo

theory

set of tested hypotheses that gives you an overall explanation of some part of nature

nature law

a statement that expressed generally observed behavior

scientific notation

method for making very large or small numbers more compact and easier to write

units

tell us what scale or standard is being used to represent the results of measurements

the two major systems of measurements

English and metrics

fundamental SI units

mass (kilogram/kg), length (meter/m), time(second/s), temperature (kelvin/k)

1 cm³ = ?

1 mL

3 major types of measurements

length (meter/m), volume (liter/l), mass (kilogram/kg)

sig figs

any measurement that involves an estimate, there will be a degree of uncertainty

nonzero integers (ex. 1759)

it IS a sig fig, example has 4 sig figs

leading zero (ex. 0.0045)

NOT a sig fig, example has 2 sig figs

captive zeros (ex. 1.005)

IS a sig fig, example as 4 sig figs

trailing zeros

YES (only when number written with a decimal, ex. 100. has 3 sig figs)

NO (100 has 1 sig fig)

exact numbers

numbers not obtained from measuring but determined by counting

sig fig is unlimited

rounding sig figs multiplication/division

round to number with smallest number of sig figs (ex. 4.56 × 1.4 you round with 1.4)

rounding sig figs w addition of subtraction

limit with number with smallest number of DECIMAL places (12.11+18.0 you would use 18.0 for reference)

temperature scales

celsius, kelvin, fahrenheit

temperature information

density

how tightly packed matter is

types of matter

Gas, liquid, solid

density = ?

D = M/V

mass = ?

M = D x V

volume in density = ?

V = M/D

density layer rules

the more dense a liquid is = further down solution

the less dense a liquid is = further up

matter

anything that has mass/takes up space

solid state

rigid; fixed shape and volume

liquid state

definite volume and takes shape of it’s container

gas

has no fixed volume or shape ; takes shape/volume of its container

physical property

qualitative observations

chemical property

ability to form or react

physical change

change in physical property

chemical change

substance turns into a different substance

element

can’t be broken down into other substance by chemical means (ex. Fe, Cu)

compound

formed when two or more elements combine chemically (ex. NaCl)

mixture

when you combine two or more pure substances physically

pure substance

contain one single element or one single compound

homogenous mixture

same throughout (uniform in composition)

heterogenous mixture

has different properties

distillation

process of boiling a solution to produce steam and collecting/cooling steam into collection flask

filtration

process of separating a liquid from a solid w/ a filter

separates a liquid from a solid

Dalton atomic theory

1. elements are made of tiny particles called atoms

2. all atoms of a given element are different from those of any other element

3. atoms of one element can combine with atoms of other elements to form compounds

4. atoms are not destroyed/created

law of constant composition

a given compound always has the same composition, no matter what

atomic number

number of protons/neutrons of an element

mass number

number of protons/neutrons of an element

isotope

atom with same number of protons but different # of neutrons

Isotope form

periodic table

shows all known elements in order of increasing atomic mass

metalloids

elements that have some metallic and some nonmetallic properties

periods

left and right of period table

groups

up and down of period table

family

ground of elements that are similar

alkali metals

group 1

alkaline earth metals

group 2

halogens

group 17

noble gases

group 18

properties of metal

efficient conduction of heat and electricity

malleability

ductility

shiny

diatomic molecules

BrINClHOF

allotropes

different forms of a given element

formation of ions

gain/lose electrons

metals tend to ___ one or more electrons to form positive ions called _

lose, cations

cations

when electrons are lost to form positive ions

named by using name of parent atom

anions

nonments gaining one or more electron to form negative ions

how do you name anions?

using root of atom followed by suffix -ide

type 1

metal present forms only one cation

type 2

metal present can only form two or more cations w/ different charges

charge on the metal ion must be identified with roman numerals

how to name type 1 ionic compounds

cation named first and anion second

cation name stays and anion is “ide”

NaCl - sodium chloride

how to name type 2 ionic compounds

cation is always named first and anion second

cation can assume more than 1 charge, charge is roman numeral in parenthesis

ex. CuBr - Copper (i) bromide

naming nonmetals + nonmetal

first element is named with full name

second element is named as if was anion “ide”

use prefix to show atoms present

NEVER USE MONO FOR FIRST ELEMENT

naming acid with NO OXYGEN

prefix “hydro” and suffix “ic”

naming acid WITH OXYGEN

acid form from root name with ic or ous (polyatomic)

ate —> ic

ite —> ous

precipitation

a chemical process that produces a solid

precipitate

solid that forms in a reaction

4 driving forces

formation of solid, water, gas, and transfer of electrons,

strong electrolyte

substance whose each unit produces separated ions when dissolved in water

molecular equation

shows the complete formula of all reactants and products

ex. AgNO3​(aq)+NaCl(aq)→AgCl(s)+NaNO3​(aq)

complete ionic equation

all substances that are strong electrolytes are represents as ions

ex. Ag+(aq)+NO3−​(aq)+Na+(aq)+Cl−(aq)→AgCl(s)+Na+(aq)+NO3−​(aq)

spectator ions

ions that do not participate directly in a reaction

net ionic equation

includes only components that are directly involved in reaction (shows major product)

ex. Ag+(aq)+Cl−(aq)→AgCl(s)

strong acid

strong electrolyte that produces H+ ions (protons) when dissolved

strong base

produces OH- in water

oxidation

OIL - oxidation is loss of electrons

reduction

RIG - reduction is gain of electrons

oxidation-reduction

a reaction that involves a transfer of electrons

reaction between metal and nonmetal

when can two nonmetals undergo an oxidation reduction reaction?

looking for O2 as a reactant or product

precipitation reaction

forms a solid when two solutions are mixed

is double replacement rxn

double replacement reaction

AB + CD —> AD + CB

acid-base reaction

H+ ion that ends up in the product as water

ez. HCL + KOH —> H2O + KCL

combustion reaction

adding oxygen and creating carbon dioxide and water

C4H10+O2 —> CO2 + H2O

single replacement reaction

A +BC —> B +AC

decomposition reactions

occurs when a compound is broken down into simpler substances

ex. 2H2O —> 2H2 + O2

synthesis reaction

reactants are elements

A + B —> C

average mass

total mass of items / # of items

1 atomic mass unit (amu) = ?

1.66 × 10^-24

mole number

6.022 × 10^ 23

def of mole

a sample of an element with a mass equal to that element’s average atomic mass

empirical formula

simplest whole number ratio