Chem all units 10th grade

Ionic

Bond between two ions of opposite charges one a nonmetal the other a metal.

Covalent Polar

Bond between nonmetals neutrally charged when electronegativity is larger than .4. Does not share electrons evenly, (sharing but one pulls more).

Covalent Non-polar

Bond between nonmetals neutrally charged when atoms share electrons evenly. Electronegativity less or equal to .4

Lewis Dot Diagram

Way to draw valence electrons and show how things will bond to each other.

Intermolecular Forces

The forces that exist between molecules, which hold them together

Dipole-Dipole

Occurs in polar molecules; attraction from polarity.

Hydrogen Bonding

Very strong dipole from the positive hydrogen. (only happens with F O N) stronger the more times hydrogen is bonded with these

London Dispersion Forces

The natural attraction of partial positive and partial negatives of protons and electrons.

Matter

anything that has mass or occupies space

Solid

A phase of Matter which has a definite shape and a definite volume

Liquid

A phase of Matter which has a shape that is dependent on its container and a definite volume independent of its container

Gas

A phase of Matter which has no definite volume of definite shape

Condensation

Gas to liquid

Freezing

Liquid to Solid

Deposition

Gas to Solid

Melting

Solid to liquid

Evaporation

Liquid to Gas

Sublimation

Solid to Gas

Non-Newtonian Fluid

Can act as either a solid or liquid depending on the force/pressure applied to them

Atom

Building block of matter

Element

Pure substance that is composed of only one type of atom

Monatomic element

Element is made up of only one atom

diatomic element

Element is made up of two of the same atom

Compound

Pure substance that is composed of two or more different types of atoms

Pure substance

Substance made up of only one element or only on compound

Mixture

When two (pure) substances are mixed together

Heterogeneous mixture

Composition is not uniform

Homogeneous

Composition is uniform

Physical change

a change in the physical properties of the matter without changing the substances in it

Chemical change

A change in the chemical properties of one or more substances. A new substance with new properties is created.

Evaporation

technique used to separate a solid dissolved in a liquid

Distillation

Technique used to separate a mixture of liquids

Filtration

Technique used to separate an undissolved solid in a liquid

Proton

Positively charged, and weigh 1 amu

Neutrons

Neutrally charged, and weigh 1 amu

Electrons

Negatively charged, and weight 0 amu

Subatomic particles

particles that create the structure that hold atoms together

Isotope

Versions of the same element that have a difference in atomic weight, either 1 more neutron or 1 less neutron

Ions

Elements with differences in charge

Cation

Loosing electrons, causes a positive charge

Anion

Gaining electrons, causes a negative charge

Valence electrons

Electrons on the outermost shell and most likely to be gained or lost

Octet Rule

Valence electrons want to be in pairs of 8

Excited state

When an electron jumps up to the next level or shell due to an increase in energy

Organic Chemistry

The study of carbon compounds

hydrocarbons

Carbon atoms with hydrogen atoms attached to them.

Alkanes

Carbons single bonded to each other

Alkenes

Carbons with double bonds in the chain

Alkynes

Carbon chain with at least one triple bond

prefixes

used to say how many carbons are in a chain

second prefix

after the prefix before the ane/ene/yne

Functional groups

groups of atoms that have similar properties and attach to hydrocarbons in specific ways

Halides

When a F, Cl, Br, or I bond to a carbon in a chain

Alcohol

when and OH bonds in a carbon in a chain

Aldehydes

When an o double bonds the end carbon in a chain

ketone

when an oxygen is double bonded to a carbon in the middle of a carbon chain

Organic acids

when a oxygen is double bonded to a carbon and also bonded to OH

Ether

A oxygen that bonds to two carbon chains

Ester

A double bonded oxygen to a carbon that’s bonded to another oxygen that is bonded to another carbon chain

Amine

a nitogen bonded to two carbon chains (usually with a hydrogen also bonded)

Amide

A nitrogen bonded to two carbon chains with one with a double bonded oxygen. (usually with a hydrogen also bonded to the nitrogen)

Symbol

A combination of letters to tell us what element we are talking about

Subscripts

The numbers at the bottom right of the symbols that tell us how much what element makes up a compound

Coefficients

Tell us how many compounds or elements there are

Neutral Compounds

How atoms combine

Periods

Rows of the Periodic Table

Groups

Columns of the Periodic Table

Alkai Metals

Group one

Alkali Earth Metals

Group Two

Halogens

Group 17

Noble Gasses

Group 18

Metaloids

Diagonal from group 13 to 16 in the periodic table.

Transition metals

D block of the periodic Table has multiple charges

Atomic Radius

The radius of an atom or width from center to edge

Ionic Radius

Radius of an ion (Atomic Radius but with an ion)

Ionization energy

Energy required to remove an electron

Electronegativity

The tendency for an atom to hold onto an electron more strongly than other atoms

Effective Nuclear Charge

Amount of Positive pull from the protons in the nucleus of an atom

Chemical equation

A mathematical way to show when things are built or broken in chemistry

Law of conservation of mass

Matter is not created or destroyed

Synthesis reaction

A reaction in which two simple elements combine to build a compound

Decomposition reaction

A reaction in which a singular compound is broken into its basic elements

Single Replacement

A reaction where a compound and an element swap spots with similar ions

Double Replacement

A reaction where two compounds combine together and swap ions from each compound

Freebie chose the number 3

3

Average Atomic Mass

Multiplying mass by relative abundance and then adding them

(mass of element/ total mass of compound )*100

Percent Composition by Mass

Molecular Formulas

The specific formula of a compound as it exists in nature

Empirical Formulas

The simplest whole Number ratio for a chemical formula

Combustion

Burning hydrocarbons, which requires oxygen, and produces CO_² and water vapor

Incomplete combustion

Combustion that creates carbon monoxide instead of Carbon dioxide

Qualitative Measurements

Subjective measurements based on what you see, hear, smell, or feel

Quantitative Measurements

Objective and numeric

Metric System

A Measurement System that is most used in science and is based on multiple of 10

Scientific Notation

A method to write our really large or really small numbers using a factor of ten

Significant Figures

How we display our answers in chemistry base upon the accuracy of a measurement

Round to the least amount of decimals

Significant Figures in Addition

Round to the least amount of significant Figures

Significant Figures in Multiplication and division

Mole

Unit of measurement that describes a certain number of atoms or molecules

Solubility Curves

Shows the relationship between temperature and Solubility