like chemsitry

like bruh

alkali metals

first row +1

alkali earth metals

2nd +2

group 13

+3

chalcogens

16th row (3rd row from left) (-2)

halogens

17th row (2rd row from left) (-1)

noble gasses

last row 0

atomic theory

everything is made of atoms and its proportional

finding moles

divide by grams to get mol/gram then avacoados number

finding mass % of molecule

divide big part by little part which is giving you a precentgae of that big part (11% of 88%) then you can multiply by big part and add them together

metal

everything except hydrogen and the line on the right

nonmetal

hydrogen+far right

metalloids

near zig zag

column v rows

up/down or left/right

1A

react with water

16

diatomic

18

unreactive

isotopes (same element)

same # of protons, different neutrons (mass)

calculating atomic mass

x time xx.xx%

joseph proust

1750-1825- fixed proportions law, constant ratio

polyatomic or mono
atomic/molecular

CHARGED (neg/pos) compound with multiple atoms
singular/plural elements

empirical formula

ratio

all ionic compounds

moecular formula

actual # of atoms

structural
ball+stick
space filling

diagram
drawing
- spaced by lines which represent how they combine
-same as above but elements are together

formula unit

two atoms combined (ionic bond, molecules are lost)
metals + non metals
lattuce

usually solid

molecular compound

when a molecule compound is formed by sharing eletron ((covalent bond))
non metals

monoatomic

1 atom

zinc

+2

aluminium

+3

silver (ag)

+1

how to charge on ion

crisscross

molcular

both names (unless 1) (dont need to include if exception)

-ate

more oxygen (1 more)

-ite

less oxygen (1 less)

ion form

-ide

naming acids

add hydro
ic
acid

oxyacids

contain hydrogen oxygen + one other element

oxyacids

1. Omit “hydrogen”

2. Start with the root name of the anion

3. Replace –ate with –ic, or –ite with –ous

4. Add “acid”

caculating molar mass

mass (g) by its molar mass (g/mol):

exocytosis

using brain cells

calcuate moles

mass/molar mass

because it has different weight

“bunch”

How many moles of Ca are in 3.01 × 10²³ atoms of calcium?

3.01×10²³ ca atom x 1 mole ca/ 6.022×10²³

amu to g/mol

same

molar mass

moles=compound

convert to moles

find molar mass and how many grams times the frequency of the molecule (a specific moleclue)

calculating # of atoms

use molar mass to find TOTAL
then multiply grams by molecule to find g/mol (moles)
then multiply by avacdos # for multiply

converting to emprical formula

assume 100

divide by mass
divide by the smallest #

scientific law

tells some aspect of the natural world

theory

explanation for something (what makes the most sense) based on laws

mixtures

physically combined (no bond/not compound)

vary in ratio

diatomic

n, h, o, i, br, cl, f,

polyatomic

s, p, o

plum pudding model

space in-between atoms

decritos

first atom- 400 BCE

dalton atomic theroy

tiny indusctible atoms
same # of protons

whole number ratio

nuclear model

mostly empty

isotopes

neutrons

name-mass

molecular vs empircal

actual vs simple

resonance strucutures

structures that have different bonds for different areas

ionic vs covalent

non metal/metal cation =metal, anion-=non. covlent= non metals

solving compounds

find charge on nonmetal to find charge on metal.

empirical formula

convert to moles.

how to calculate

be smart (divide by fraction=big, show how mass total goes to mass then grams)

limiting reagent problems when finding the final product

use the limiting reactant before dividing to calculate how much that makes