Chemistry in a Nutshell

Chemistry

branch of science that deals with the study of matter and the ways in which different form of matter combine with each other

element

a substance that cannot be broken down into any substance and made with its own type of atom

compound

a molecule made from two or more different element that have been chemically joines (ex. H₂O and NaCl)

molecule

two or more atoms connected by chemical bonds which form the smallest unit of a substance that retains the composition and properties of that substance

mixtures

a physical combination of two or more substances that aren’t chemically joined

homogenous mixture

is a mixture that has the same composition throughout

heterogenous mixture

a mixture with distinguishable features and not spread throughout

solution

a homogenous mixture with tiny particles that are too small to see and filtered out of the mixture

colloid

homogenous mixture with medium-sized particles that are large enough to see but not large enough to settle

suspension

heterogenous mixture that is large enough to see and to settle and be filtered out of the mixture

matter

is anything that occupies space and has mass

plasma

an extremely hot, ionized gas; compromised of negatively charged atoms and positively charged atoms

Bose-Einstein condensate

forms at temperatures near absolute zero Kelvin, without additional energy to transfer, the atoms began to clump into a super-atom

Quark-gluon plasma

forms at extremely high temperatures that are so hot, the individual quarks

degenerate matter

an extremely denser state of high energy atter found in the heart of neutron stars and white dwarfs

liquid

a substance that retains its size and shape of a container; has definite volume but no definite shape

solid

substance that retains its size and shape without a container; has definite shape and volume

gas

substance that can move freely and can take the shape of the container; has no definite shape and volume

melting

phase change where solid turn to liquid

freezing

phase change where liquid turns to solid

evaporation

phase change where liquid turns to gas

condensation

phase change where gas turns to liquid

sublimation

phase change where solid turns to gas

deposition

phase change where gas turns to solid

intensive property of matter

properties of matter that does not depend on the size or quantity of matter in any way

intensive property of matter

odor, color, melting point, ductility, malleability, electric conductivity, pressure, boiling point, luster, freezing point and density is an example of what properties of matter?

extensive property of matter

properties of matter that depends on the system size or the amount of matter on the system

extensive property of matter

mass, length, weight, and volume are example of what properties of matter

atomic number

the number of protons in an atom is referred as?

isotopes

forms of the same atom that differ only in their number of neutrons

isomers

forms of the same molecule that differs only in its structure

allotropes

forms of the same element that differs only on its physical appearance

atomic mass

simply the total mass of an atom that is generally expressed in atomic mass unit (amu)

radioisotopes

process of isotopes in which they release, emit, kick out, subatomic particles to reach a more stable, low energy configuration

decay

process in which radioisotopes release particles and energy

half-life

period in which half of the material will decay to a different, relatively stable product

subatomic particles

particles smaller than atoms

protons, neutrons, electrons

what are the three subatomic particles

protons

origination of positive charges of an atom

electrons

negatively-charged atoms found outside the nucleus

neutrons

neutrally-charged subatomic particles

Ernest Rutherford

discovered the proton’s existence in 1919 when he projected alpha particles in the gold foil and the positive alpha particles were deflected

Sir John Joseph Thomson

discovered the electrons in 1897 after experimenting involving cathode rays

electrons, protons - neutrons

___________ have less mass than _________ and ________.

ions

are produced if the number if protons and electrons are unequal

cations - anions

positive ions are _______ while negative ions are ________

James Chadwick

discovered neutrons when he demonstrates a penetrating radiation incorporated beams of neutral particles

ionic compounds

formed when metal compounds lose one or more electrons to nonmetal atoms

molecular compounds

inorganic compounds that take the form of discrete molecules

chemical formula

expression that shows the elements in a compound and the relative proportions of those elements

combination reaction

also known as synthesis reaction; it is a reaction in which two ir more substance combine to form a single new substance

combination reaction

A + B = AB

decomposition reaction

decomposition reaction

AB —> A + B

single replacement method

reaction in which one element replaces the similar element in a compound; happens mostly in the interswitch of metals and nonmetals

single replacement method

A + BC —> AC + B

double replacement method

reaction in which the positive and negative ions of two ionic compounds exchange places to form two new compounds

double replacement method

AB + CD —> AD + BC

combustion method

is a reaction in which a substance react eith oxygen gas releasing energy in the form of light and heat, it must involve oxygen as a reactant as well as hydrocarbons

hydrocarbons, carbon dioxide - water

in a combustion reaction, ________ react with oxygen gas to form _______ and ______.

H₂, N₂, O_2, F₂, Cl₂, Br₂,and I₂

What are the seven diatomic molecules that exist in nature?

mole

it is the SI quantity for chemical entity

6.022 × 10²³

Avogadro’s number that states the absolute number of elementary entities in one mole

molar mass

the mass of a given substance divided by its amount of substance presented in g/mol

valence electrons

are the electrons found in the outermost shell

subshells

consist of s-subshell. p-subshell, and more; it determines the placement of electrons from the nucleus

principal values

also referred as the periods in the periodic table; the horizontal array of elements that determines the subshell of an atom

electron configuration

refers to the arrangements of electrons in an atom

non-metals

these are anions with negative charge (ex. H, C, N, O, P, S, Se)

metals

cations with positive charge

halogens

these are chemical elements that forms salt when reacted with nonmetals (ex. F, Cl, Br, I, As, Ts)

atomic element

an element represented with no subscript (ex. Fe)

molecular compound

compound made up of two nonmetals

ionic compound

compound made up of a metal and a nonmetal

molecular element

a substance made of atoms of the same element

Stock system

a formal and modern distinction of naming an ion by using roman numerals (ex. iron (iii) ion)

Classical/Common name

prelavent distinction of naming ions majorilly used in health science (ex. ferric ion)

-ic, -ous, -ide

cations use suffix ____ if it uses three or more cation charges and _____ if it uses two charges, however the suffix ____ ide is used for anions

acid

a molecular compound that contains one or more hydrogen atoms and produces hydrogen ions when dissolved in water

binary acid

an acid that consists of a hydrogen and one other element mostly halogens

hydro - (base name of nonmetal) - ic + acid

how do we name binary acid?

oxyacid

an acid that contains a hydrogen, an oxygen, and a third element, mostly nonmetal

Boron group

elements who belong in group 13 or Group3A and classified as metalloids having properties of both metals and nonmetals

Carbon group

elements that belong in Group 14 (ex. carbon, silicon, tin, and lead)

Nitrogen group

elements that belong in Group 1 or 5A (ex. nitrogen, phosphorus, arsenic)

halogens

elements in group 17 or Group 7A; they are reactive non-metals that form very acidic compounds with hydrogen to form simple salts (-ine elements)

Chalcogens

elements in Group 16 or group 6A (ex. oxygen, sulfur, selenium)

noble gases

occupies group 0 or group 18 and known to be unreactive because they are stable and follows an octet rule (except hydrogen) (ex. hydrogen, argon, neon, krypton. xenon, radon, organesson)

metals

the one highlighted as blue in the periodic table is considered as ___________

metalloids

the one highlighted as green in the periodic table is considered as ___________

nonmetals

the one highlighted as red in the periodic table is considered as ___________

7 periods and 18 families

how many periods and families does the periodic table have?

electronegativity

ability of an atom to attract electrons in a chemical bond

electro-positivity

ability of an atom to lose electrons

increases

the electronegativity of an atom _______ from lowest group to the highest group

decreases

the electronegativity of an atom _______ from lowest period to the highest group

florine

it is the most electronegative element

cesium

it is the most electropositive element

intermolecular forces

basically knows as the attractive and repulsive forces that arise between the molecules of a substance; dependent reason why physical and chemical changes occurs