Chapter 2: Atoms, molecules, and ions

Question 1

Law of multiple proportions by dalty-poo

Answer 1

elements forming a series of compounds will always have a ratio of the second compound to the first that reduces to whole numbers (basically in CO vs. CO2, oxygen ratio can be reduced down to 2:1, and in CO2 vs. CO3, oxygen can ratio can be 3:1)

Question 2

law of definite proportions (proust)

Answer 2

compounds always contain same proportions of elements by mass (basically means this many atoms to this many atoms per compound)

Question 3

Dalton’s atomic theory (highly unlikely to be in test)

Answer 3

1. every element is made of atoms
2. atoms of an element are all identical to each other, and different to atoms of another element
3. chemical compounds = atoms of diff. elements combined, same relative # and types of atoms (see laws of proportions)
4. Chemical reactions = reorganization of atoms/bound together, not atoms themselves

dalton was not entirely correct

Question 4

Avogadros hypothesis

Answer 4

same temp, pressure, and volume = same number of particles

Question 5

Thomson cathode ray something something something

Answer 5

made a ray and stuff and hypothesized it was, like, kinda made of electrons, or something, then did it from various types of metals, made plum pudding model of atom

Question 6

Rutherford gold foil experiment

Answer 6

guy shoots some alpha particles at a thin metal foil, most pass through, some points are scattered, but others entirely reflect past detector

the big boy reflections had to mean something else positive was at the center of an atom, created nuclear atom model (nucleus and electrons somewhere around it)

Question 7

atomic number vs. atomic mass

Answer 7

atomic number is what modern periodic table organizes by, = amount of protons, atomic mass = total number of protons + neutrons, electrons have no mass tho and when removed or added become ions

Question 8

what maketh an isotopes

Answer 8

Isotopes are atoms with more or less neutrons than the original

Question 9

ionic bonds ?

Answer 9

yes they are because cation and anion attract and share electron (ex. NaCl)

Question 10

salts

Answer 10

ionic compounds that are ((usually)))) solids

Question 11

Binary Ionic compounds (types I, II, and III)

Answer 11

in all ionic compounds there is a positive ion which is always written first and negative ion which is written second (and if anion is only one atom, add -ide ending)

type I is just basic cation name + anion name with -ide ending
Type II is the charge of a transition metal + anion with -ide ending (ex. iron (II) chloride)

Question 12

different oxygen levels of polyatomic ions

Answer 12

uses system from least to greatest as follows: hypo(insert ion name here)ite, (ion name)ite, (ion name)ate, and per(ion name)ate

NOTE: not all polyatomic ions have 4 different oxyanions (anion w/Oxygen in it)

Question 13

Covalent/molecular compounds

Answer 13

DO NOT CONTAIN IONS, BONDS FORMED COVALENTLY

First element named first, then second named with -ide, w/prefixes to determine number (but mono is never used on first element)
(ex. dinitrogen monoxide, carbon monoxide)

Question 14

What tips you off that something be an acid

Answer 14

H+ ion/H at the beginning of the chemical formula name

Question 15

how do you name an acid w/o oxygen (ex. HCl)

Answer 15

use hydro prefix, -ic, and acid (ex. hydrochloric acid)

Question 16

Name acids WITH oxygen based on ite or ate endings: (ex. HClO2 and HClO3)

Answer 16

Ite endings result in being an -ous acid (no hydro) (ex. HClO2 = Chlorous acid

Ate endings result in an -ic acid (no hydro) (ex. HClO3 = Chloric acid)