Electrons
The minimum amount of energy that can be gained or lost by an atom.
quantum
How the modern periodic table is arranged
By atomic number
Atomic radius/ atomic size
What is half the distance between two adjacent nuclei
What occurs in an ionic bond
Transfer of Electrons
What happens in a covalent bond
Electrons are shared
metallic bonds model
Sea of Electrons
Polar covalent bond
A type of bond that forms when electrons are not shared equally
photon
A quantum of light (A particle of electromagnetic radiation with no mass that carries a quantum of energy)
The way a period is organized on a periodic table
Across or horizontal
Electronegativity
The ability of atoms to attract an electron.
What is the trend?
Increases going across; decreases going down
Fluorine is high point
Formula unit
Simplest ratio of a chemical formula for an ionic compound
The name for a product of a covalent bond
Molecule
delocalized electrons
The electrons involved in metallic bonding that are free to move easily from one atom to the next throughout the metal and are not attached to a particular atom
H + 7
Memory trick for remembering the 7 diatomic gasses that are joined by covalent bonds. The list includes: H2,N2,02, F2, Cl2,Br2, I2
Bohr Model description
Limits the electrons to a certain path or value or quanta. Bohr model describes electrons in certain paths or circular orbitals.
On the left, along the stair step, and on the right respectively
Ionization energy
The amount of energy it takes to remove an electron
Trend:
increases going across: deceased going down
valence electrons
The electrons in an atoms outermost orbital that determine its characteristics. These are the electrons that participate in the chemical reaction.
Number of electrons involved in a single, double, triple bond.
2, 4, 6
Examples: Cl2, 02, N2
alloy
A mixture of elements that has metallic properties; most commonly forms when the elements are either similar in size (substitutional alloy) or the atoms of one element are much smaller than atoms of the other (interstitial alloy) Makes a material that has quality superior to the elements that make it up.
The amount of energy required to break a specific covalent bond
bond dissociation energy
Quantum mechanical model description
Limits electrons to a certain quanta. The quantum mechanical model describes the probability of an electron being found within a particular volume of 3D space around the nucleus or in an orbital. This is the modern atomic model. (disproves Bohr model)
The names of groups one and two on the periodic table
alkali metals and alkaline earth metals
How anions and cations are formed
Anions gain electrons; cation lose electrons. They do this to satisfy the octet rule. Follow up question: How does ion formation change atom size?
Number of valence electrons in each group
group 1 has 1
group 2 has 2
group 13 has 3
group 14 has 4
group 15 has 5
group 16 has 6
group 17 has 7
group 18 has 8
Characteristics of molecules
Solid, liquid, or gas at room temperature; lower melting point than ionic compounds, poor conductors of heat and electricity.
Examples of alloys
14 karat gold, brass, stainless steel, cast iron, and others
Relationship of bond dissociation energy to the strength of covalent bond
The shorter the bond,the stronger the bond. The more electrons involved in a bond, the stronger the bond. The stronger the bond the more dissociation energy needed to break it.
why hot things glow
Electrons are excited by the heat. They make a quantum leap to a higher energy level. When they cool off and return to the lower energy level, they give off a photon of light that is characteristic of their element.
Group numbers 3-12, 17, 18
Explanation of the trend of atomic size decreasing across the periodic table
Protons and Electrons are added in each element as you go across the periodic table creating more positive and negative attractive charges which pull the electrons in closer to the nucleus.
Characteristics of ionic compounds
Crystalline, crystal lattice, high melting point and boiling point, brittle, hard, conduct heat and electricity only when melted or in dissolved
VSEPR model
Valence Shell Electron Pair Repulsion model, which is based on an arrangement that minimizes the repulsion of shared and unshared (lone) pairs of electrons around the central atom.
characteristics of metals and reason for the characteristic of metals
Good conductors as solids, malleable, ductile.
These characteristics are due to the delocalized electrons in the metallic bond
Description and explanation of the three intermolecular (between molecules)forces
Induced dipole occurs between non-polar molecules due to movement of the electrons; it is a temporary bond. Dipole-dipole forces occur between oppositely charged regions of polar molecules. Hydrogen bonds are a strong intermolecular attraction between molecules that contain an hydrogen atom bonded to a small highly electronegative atom like oxygen, nitrogen, or fluorine.