Chemistry Unit 1-1

Matter

anything with mass that takes up space

building blocks of matter

atoms

number at the top of each box on periodic table

atomic number/number of protons

number of protons =

number of electrons

number at the bottom of each element

atomic mass

non-metals (location)

step stool starting to the left of B (boron)

table numbered by (protons or atomic mass)

protons

metals (location)

to the left of Boron step stool

metalloids

B, Si, Ge, As, Sb, Te, Po, At, Lv, Ts

properties of metals

lustrous, malleable and ductile, very conductive, solid at room temp except Hg, typically cations

non-metals

waxy or dull appearance, brittle, poor conductors, solid or gas form at room temp except Br, typically anions

cations

positive charge (lost electron(s))

anions

negative charge or gained an electron

ion=

charged atom (lost or gained electrons)

periods

7 rows called periods

families/groups

18 columns called families or groups, elements in the same group have similar properties and the same number of valence electrons

also tend to have the same charge

metalloids/semimetals

combination of properties between metal and non-metal

first element is a non-metal

covalent compund

first element is hydrogen

acid

first element is metal

ionic compound

binary ionic compound

compound result of metal and non-metal react to form a cation and an anion

metals and non-metals (during a reaction)

typically metals transfer electrons to non-metals

metals become cations and non-metals become anions

cations and anions _____ forming ____

attract each other (electrostatic force of attraction between oppositely charged ions)

an ionic bond

formula unit

simplest representative particle of an ionic compound (ex. NaCl)

formula unit charge is ___

neutral, total positive charge cation = total negative charge anion

monoatomic ions

most elements follow a trend

Alkali metals

tend to form +1-lost an electron

soft

explode when exposed to water

most reactive metals

group 1

Alkali earth metals

group 2

tend to form +2 - meaning they lost 2 electrons

less reactive than group 1, harder metals

transition metals

(3-12) no trend

except aluminum which is +3

inner transition metals

bottom part, no trend

noble gases

group 18

inert, 0 charge, do not bond

halogens

group 17

most reactive non-metals

tend to form -1 ions

naturally occur in diatomic form (2 of the same combined)

oxygen group charge

-2

nitrogen group charge

all elements left of the step stool form

cat ions

to the right of the step stool always form

anions

hydrogen is technically a part of the ____ group

halogen

polyatomic ions

compound with 2 or more nonmetals with a charge

per and hypo and ate and ite tell us

ate = higher number of oxygens

ite = lower number of oxygen

per- = lowest

hypo- = highest

criss cross method

lowest common multiple then reduce

naming of ionic compund if first element is a metal without a Roman numeral

nonmetals - root of name +ide

nonmetals

F = fluoride

Cl = chloride

Br = bromide

I = Iodide

O^-2 = oxide

S^-2 = sulfide

N^-3 = nitride

P^-3 = phosphide

hydrate

when water is attached to an ionic compound

prefixes

mono 1

di 2

tri 3

tetra 4

penta 5

hexa 6

hepta 7

octa 8

Nona 9

deca 10

Acids have to be in ____ state

aqueous state

Acids start with

H

Binary acid is how many elements

2

Acid-

a compound containing hydrogen and either a nonmetal or a polyatomic ion in the aqueous state

Binary acid naming

Hydro prefix + root of the second elements name + ic acid

EX hydrofluoric acid

Ternary acid naming

no hydro

if the polyatomic ion ends in ate it is substituted for ic

if ion ends in ite it is substituted for ous

ternary acid consists of

covalent compound

contains 2 or more nonmetals bonded in a specific way

covalent compounds formula

prefix for number of atoms of first element then name + prefix for number of atoms of second elements then name with ide ending

ao→o

oo→o

alkanes hydrocarbons

1 carbon meth

2 eth

3 pro

4 but

5 pent

6 hex

7 hept

8 oct

9 non

10 dec

all followed by ane

Applied Research

Applied research is a type of research that seeks to solve practical problems by applying scientific theories and principles. It focuses on real-world applications and aims to improve processes, products, or services.

Physics

Physics is the natural science that studies matter, energy, and the fundamental forces of nature. It seeks to understand the behavior of the universe through concepts such as motion, force, energy, and the structure of atoms.

Alkanes

Alkanes are a class of hydrocarbons consisting of carbon and hydrogen atoms, characterized by single bonds. They follow the general formula CnH2n+2 and are saturated, meaning they contain the maximum number of hydrogen atoms.

alkenes (not for test 1)

at least 1 double bond and has ene ending

alkynes (not for test 1)

at least 1 triple bond

ends with yne

alcohol

O-H on the end

e is removed from end and ol is added instead in the name

carboxylic acids

COOH group

replace e with -oic acid in name

A Law is

Summarizes a generally observed behavior or phenomenon in nature that can’t be disproved

“what happens”

A theory is

Explains how or why a phenomenon or behavior in nature occurs

“why something happens”

Law of Multiple Proportions Test

set one element = to 1g

make ration of element 1 to element 2

makes a ratio

6 parts of Dalton’s atomic theory

each element is composed of tiny individual particles called atoms

atoms are indivisible, they cannot be created or destroyed

all atoms of an element are identical and have the same properties

atoms of different elements have different properties

Atoms of one element may combine with atoms of other elements in whole number ratios to form molecules

Each molecule always contains the same type and number of atoms.

Radioactive particle charges

radiation = high energy particles

positive charge = alpha particle

negative charge = beta particle

neutral charge = gamma particle

cathode ray tube lead to the discovery of

plum pudding model + electrons

plum pudding model had a positive cloud with negative particles randomly distributed in the cloud, had a neutral charge

rutherford gold foil experiment

most positively charged alpha particles went through the gold but some were deflected, disproving the plum pudding model where all should have gone through

small dense positive mass in the middle deflected a few of the particles, leading to the discovery of the nucleus

mass of electron, proton, neutron

no mass, 1amu, 1amu

do not need to know mass in grams

proton/neutron mass in g = 1.67×10^-24

electron mass in g = 9.11×10^-28

molecule def

2 or more same or different atoms bonded together in a specific way

IMFs

Intermolecular forces, determines the state of matter

change in intermolecular force (state of matter) is a physical change

chemical bond def

intramolecular forces are forces between two atoms making them act as a unit, chemical change (change to the composition of the matter), make a new type of matter

physical properties include

Melting and boiling points, viscosity, magnetism, density and conductivity, Color, shape, state of matter, appearance, smell, taste

chemical property

describes the chemical reactions of a pure substance - what an element or compound can do

chemical properties cannot be observed just by looking at the matter, a change has to take place

a change to the substance that changes its composition, causing a new substance to be formed

usually cannot get back the original substance

physical change

can get back substance

ex freezing, melting, dissolving, boiling

ISOTOPES

TWO OR MORE ATOMS WITH THE SAME NUMBER OF PROTONS BUT A DIFFERENT NUMBER OF NEUTRONS, same element different mass number