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Bonds-Hold compounds together. Atoms form bonds in order to have 8 valence electrons.
Ionic Bonds-Transfer of electrons between atoms. Between Metals and Non-metals. Positive and negative charge attract the atoms together.
Covalent Bonds-Sharing of electrons. Only between non-metals. Covalent bonds can share 1,2, or 3 pairs of electrons resulting in single, double, or triple covalent bonds.
Hydrogen Bonds-Covalent Bonds specifically with Hydrogen atoms. Strongest intermolecular force.
Metallic Bonds-Bonds holding metallic atoms together. They are found in the solid or liquid phases. In a metallic atom, there is a kernel of the nucleus and non valence electrons. The valence electrons move freely throughout the crystal. When force is applied, the crystal changes shape but stays intact. Metallic bonds have high conductivity due to the freely moving valence electrons. They also have high melting points and boiling points.
Polarity-The difference of electro negativity between atoms. Also the symmetry of a molecular structure. When the electronegativity values are different, the sharing of electrons are unequal. This is called polar covalent. The atom with the higher electronegativity attracts the electrons more. Non polar covalent bonds are when the electronegativity difference is 0.4 or lower.

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metalloids are found on the 'staircase'

include B, Si, Ge, As, Sb, Te

Al and Po are NOT metalloids

metals can be found to the left of the 'staircase'

nonmetals can be found to the right of the 'staircase'

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Atomic number in an atom is the number of protons.
In a neutral atom theres is the same amount of of protons and electrons.
All atoms have an electron configuration.

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Mass is neither created or destroyed
2H2 + _O2 -> 2H2O
4g + _g -> 36g
Find number of O2 used

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Atoms have protons, neutrons, and electrons. They also have a nucleus.

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Atoms have protons, neutrons, and electrons. They also have a nucleus.

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Where all of the groups and periods of elements are shown. Elements are shown along their their mass, number, oxidation states, electron configurations and are represented by a letter or two.

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Energy: ability to do work
Kinetic energy: energy of motion
Potential energy: energy of position
Temperature: measure of average kinetic energy
Heat: quantity of energy

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The electrons are negatively charged and they can be found in orbit.
Protons are positively charged and can be found in the nucleus.
Neutrons have a neutral, or no charge that can also be found in there nucleus.

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Down a group:

Atomic radius and metallic character INCREASE, electronegativity and ionization energy DECREASE

Across a row:

Atomic radius and metallic character DECREASE, electronegativity and ionization energy INCREASE

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Atom-the smallest particle of an element that can enter into a chemical reaction.
Atomic mass-the average mass of all the isotopes in a sample of an element.
Atomic mass unit-one twelfth the mass of a carbon-12 atom
Atomic number-the number of protons in the nucleus of an atom.
Compound-a substance composed of two or more elements that are chemically combined in definite properties by mass
Electron-a fundamental particle of matter having a negative charge
Element-substances that cannot be broken down or decomposed into simpler substances by chemical means.
Excited state-the condition that exists when the electrons of an atom occupy higher energy levels while lower energy levels are vacant.
Ground state-the condition of an atom or ion in which the electrons occupy the lowest availability energy levels
Heterogeneous-a mixture in which the substances are not uniformly mixed.
Homogeneous-a substance in which the particles are uniformly mixed.
Isotope-atomod an element that has a specific number of protons and neutrons.
Mass number-the total number of protons and neutrons in the nucleus of an atom.
Mixture-combination of two or more pure substances that can be separated g physical means.
Neutrons-the uncharged particle on the nucleus of an atom.
Orbital-a región in an atom in which an electron of a particular amount of energy is most likely to be located.
Proton-the positively charged particle in the nucleus of an atom.
Pure substance-a compound or an element; a material n which the composition is the same throughout.
Valence-the electrons in the outer energy level of an atom.

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Solid phase: matter that is held in a rigid form. Has definite volume and shape
Liquid phase: particles are held together as rigidly as the solid particles. Particles are able to move past each other. They don't have a definite shape, but do have a definite volume
Gaseous phase: particles have minimal attractive forces holding them together. Have neither a definite shape or volume

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Atoms are mostly made up of empty space

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Ion-An atom or molecule with a net electric charge due to the loss or gain of one or more electrons.

Malleability-The ability of a substance, usually a metal, to be deformed or molded into a different shape.
Conductivity-How well something conducts energy
Solubility-How fast something dissolves
Solute- The thing that gets dissolved
Solvent-The liquid that dissolves something
Octet-The configuration of 8 valance electrons.
Octet rule-This rule states that atoms generally react by gaining, losing, or sharing electrons in order to achieve a complete octet of eight valance electrons—the configuration of a noble gas.

Lewis Dot Diagram-Also known as an electron dot diagram, which insists if a chemical symbol surrounded by one to eight dots representing the valance electrons.

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Picture of solid, liquid, and gaseous phases

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Picture of solid, liquid, and gaseous phases

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• consists of metals and non metals
• firmed by the transfer of electrons from one atom to another
• crystal structure of positive and negative ions
• high melting points
• good conductivity of heat and electricity (as liquids)

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The amount of energy needed to remove the most loosely bound electron.

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Shows all of the elements with their names, symbols, trends, first ionization energies, electronegativities, melting point, boiling point, density, and atomic radius

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Protons and Neutrons have a mass of 1 amu while electrons weigh appropriately nothing

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• low melting points
• poor conductivity of electricity
• relatively soft

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Very dense

Colorful ions in solution

Varying reactivity

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This experiment was performed by Ernest Rutherford. He aimed a particle shooter at gold foil where the majority of the particles passed and a few deflected away. Which shows that the atom is mostly empty space with a small dense positively charged nucleus.

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Groups- 18 groups that have the sameness amount of valance electrons and go up and down on the reference table
Period- 7 periods are horizontal rows that increase consecutively by atomic number

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-Heating and cooling curves are used because pure substances can't be physical separated into their components, we can identify them through properties like density, boiling point, and freezing point. Each substance has its own unique curves.
-Heat flows from the highest temperature to the lowest.

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Qualitative Data
• Consists of characteristics seen in object
• Ex: Shape, size, color, etc.
Quantitative Data
• Data obtained by the use of instruments or by counting
• Typicaly consists of numbers
• Ex: Length/Width - use ruler
Temperature - use thermometer
Barometer - air pressure
Volume - graduated cylinder

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Table T has the mole calculations

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Atoms react when they gain, lose or share electrons (also known as bonding)

Metals lose electrons

The greater the ability to lose electrons, the more reactive

Metallic reactivity increases moving down a group

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number of units in one mole of any substance shows the molecular weight in grams), equal to 6.02 x 10^23

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Percent Error

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Atoms react when they gain, lose or share electrons (also known as bonding)

Nonmetals gain electrons

the better the nonmetal is able to gain electrons, the more reactive it is

Down a group, reactivity decreases

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A measure of the attraction of a nucleus for a bonded electron

Electronegativity values are Located in Table S

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-have both properties of metals and nonmetals
-metalloids are located on the stair step line. The two exceptions that are on the stair step line are Aluminum (Al) and Polonium (Po) which are metals

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• attraction between polar molecules
• positive area of one dipole is attracted to the negative area of another dipole

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In each period, the number of valence electrons increases from left to right, and the properties of the elements change systemically.
On periodic tables, the metalloid are located adjacent to a diagonal, stair step line.

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1) All non zero numbers count
Ex: 485 - 3 significant figures (Sigfigs)
2) A zero at the beginning of a number doesn’t count
0.00485 - 3 sigfigs
3) Captive zeros count
405 - 3 sigfigs
4) The Absent Present Rule (“Atlantic Pacific Rule”)
300
• Has 1 sigfig.
• No decimal point present, only # count
300.
• 3 sigfigs
• With decimal point, all numbers count

5) Addition & Subtration Rule
• When adding or subtracting, preform calculation THEN look at how many places beyond decimal point each of your values are. LEAST # OF PLACES BEYOND DECIMAL USED IN FINAL ANSWEE
Ex: 48.65 + 59.2 + 7.0 = 114.85 -> 115

6) Multiplication & Division Rule
• Multiply or divide as directed, then your answer will have as many sigfigs as value with LEAST NUMBER OF SIGFIGS
Ex: 45 x 4 = 180 -> 200

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Physical: no change in the identity of the substance(just different phase)
Chemical: substance changes into a new substance with new properties(new compound)

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Formula Mass: The sum of the atomic masses of a substance.

Gram Formula Mass: The sum of the atomic masses of a substance expressed in grams.

Mole: the gram formula mass is equivalent to one mole.

Percent Composition: Represents The composition as a percentage of each element compared with the total mass of the compound.
Percent Composition by Mass: (Part’s mass/Wholes's mass) x 100 **On Table T**

Avogadro’s Number: 6.022 x 10^23

Empirical Formula: The simplest form of the molecular formula.

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Polyatomic
Metals
Non metals
Hydrogen
Oxygen

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Compounds: two or more elements chemically combined. Can only be broken down chemically
Mixtures: 2 or more substances physically combined
- heterogeneous: unevenly mixed, can see 2 or more things
- homogeneous: evenly mixed(a solution)
Elements: all atoms have to same atomic number. Can't be broken down chemically
Diatomic elements: Br I N Cl H O F

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Provides a basis for the size of an atom

Equal to half the distance between 2 neighboring nuclei of the same element

As you move down a column, the number of shells increases (making the atom bigger)

As you move across, each successive element hasn’t one more proton that increases the nuclear charge

Positive charge 'pulls' on the outermost shell, making the atom smaller

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Noble gases don’t have all the properties of no metals because they are generally unreactive.
Only a few stable compounds containing noble gases have been formed.
Each of these elements has a completely filled outer energy level of electrons.
Noble gases are group 18

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1. Accuracy: a measure of how close a measurement comes to the actual or true value of whatever is measured.

2. Precision: a measure of how close a series of measurements are one to another

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• Each element within a compound has its own charge, oxidation states
• “-ide” is a chemical suffix commonly used for the second part of the name of a compound
• the above is not the be confused with “-ate” or “-ite”, which are used with anions and ions (Table E in reference table)
• oxidation states/charges are swapped between elements in chemical formulas (criss-cross method)

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An atom in the grand state absorbes energy
Excited state( unstable)  releases energy in the form of light

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Group 17

Have 7 valence electrons

Nonmetals

Gain one electron

Only group on the periodic table that has all 3 phases of matter at STP

F2 , Cl2 are gasses at room temp

Br₂ is the only liquid nonmetal at room temp

I₂ is solid at room temp

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Some no metals can exist in two or more forms in the same phase. These forms are called allotropes,

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Stated that elements are made up of mixed atoms. He said an atom was a hard indivisible sphere.

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Group 1

Metals

Have one valence electron, lose that electron to become a more stable ion

Are never found uncombined and rarely found in natural state

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-easily lose electrons
-never found in their atomic state (always in compounds)
-low ionization and electronegativity levels

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Solid at room temp (except for Hg)

Shiny, maleable (bendable)

Ductile with high melting points

Good conductors of electricity and heat

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Can be solid, liquid or gas at room temperature

Bromine is the only liquid nonmetal

Solids:

Carbon, Sulfur & Iodine (C, S, I₂)

Liquids:

Bromine (Br₂)

Gasses:

Oxygen

Neon

Fluorine

Chlorine

Nitrogen

All of group 18