(term 1) Test 3 Chemistry Info (Exam)

Chemical Formula

Represents ratio of ions in a compound.

Molecule

Single unit formed by covalent bonds.

Stereo Isomer

Same connectivity but different spatial orientation.

Nonelectrolyte Solution

Dissolves in water but does not conduct electricity when dissolved.
They do not produce ions in a solution and are similar to covalent compounds.

Cation

Positively charged ion from electron loss.

Chemical Bonds

The attractive force that holds atoms together within a compound always includes electrons, which will be attracted to their own nucleus, and nucleases of other atoms

Ionic Bond

Can be represented by a group of ions
Electrons are transferred between atoms to create ions. It means that one atom loses electrons and another atom gains electrons which creates (cation/anion). The bond is a positive charge being attracted to the negative charge of millions and billions of molecules.

Anion

Negatively charged ion from electron gain.

Covalent Bond

Can be represented by an individual molecule, not a bunch of atoms
Atoms are close together and overlap and share electron clouds
Singular units called molecules are formed from these bonds
These bonds are formed between 2 nonmetal atoms
Insoluble in water

Ionic Solids

Held by electrostatic forces (opposite attracting forces) between ions.

What structure do ionic bonds form?

crystal lattice structure

Electrostatic Attraction

attraction between oppositely charged ions.

Properties of Ionic Solids

Composed of a metal and a nonmetal = polyatomic ions
To melt them, it must be thousands of degrees because their bonds are extremely strong
This means they have a high melting and boiling point
With ionic solids, they cannot have like charges because they will repel
Atoms are locked in a hard but brittle lattice
Also resistant to being scratched

Ionic Solids (Brittle)

Something that will crumble easily, if their ions get misaligned they will fall apart

Ionic Solid (Conducting)

Poor in solid state because the ions are free to move, good when dissolved because the ions are bonded and cannot move around

Ionic Solid (Solubility)

They dissolve in water and are good conductors in this form

Electrolyte

Similar to a ionic compound that conducts electricity when dissolved, the flow of the electric current moves through mobile charged particles. It has dissolved ionic compounds have freely moving ions that can conduct electricity.
They can dissociate into ions when dissolved in water.

Strong Electrolytes

Completely dissociate

Weak Electrolytes

Partially dissociate.

Covalent Compounds

When atoms in a molecule are held together by covalent bonds.

Intermolecular Forces

Forces allowing molecules to stick together. These forces are strong, but not as strong as Ionic or Covalent bonds.

Covalent Compound Properties

Softer than ionic compounds, has low melting and boiling points, and poor conductivity. This happens because electrons are shared and they are not charged, they can never conduct electricity under any circumstances.

Metallic Compound

Similar to ionic because they have moving charged particles. Shared electrons create a 'sea' of conductivity. They are also similar to covalent bonds because they have shared electrons between all the atoms.
Involves the attraction between free-floating valence electrons (delocalized) and positively charged metal ions.

Delocalizing Electrons

Free floating valence electrons, they are not bound to any 1 atom

Metallic Compound Properties

Large range of melting points
Group I metals have very low melting points, and most will melt in your hand.
Transition metals, have higher melting points.
Shiny because they have electrons that move to the surface and when light strikes them they become shiny
Ductile and malleable
Ability to move the ions around
Opposite of brittle
Great conductors.
Metals are the only conductors that can conduct in the solid state
Do not dissolve, water cant tear it apart
It's a metal if there are elements from the left side of the table included

Electrical Conductivity

Free electrons carry electric current.

Thermal Conductivity

Electrons transfer kinetic energy.

Valence Electrons

Electrons in the outermost energy level of an atom. Responsible for chemical properties and bonding behavior.

Network Covalent Solids

Giant molecules with covalent bonds throughout.
They have a crystalline structure.
In a continuous network
Hard
Sublime or melt at high temp
Nonconductors
Examples are diamond, graphite, and quartz.
Covalent structures do not dissolve (nonsoluble)
Dont conduct electricity

Single Bond

Two electrons shared between two atoms.

Double Bond

Four electrons shared between two atoms.

Triple Bond

Six electrons shared between two atoms.

Octet

an atom with 8 valence electrons that is stable and low in energy

Duet

When 2 electrons is a full shell. It is hard for Hydrogen to get into an octet, its most stable point is a duet

Stable Molecule

When they have an octet

Dot Structure

Allows to know how many bonds are needed
These dot structures combine to form compounds that achieve the required octet or duet

Lone Pair

non-bonding, already bonded because there are more than 4 valence electrons originally
represented by dots that are not connected

# of bonds a element makes?

The distance the element is from the noble gas is the amount of bonds it will make in total, ex. Nitrogen - 3 bonds

Lewis Structures

Visual representation of valence electrons in molecules.

Functional Group

Cluster of atoms determining molecule properties.

Alkane

Has C & H with only single bonds.

Alkene

C & H with one or more double bonds.

Alkyne

C & H with one or more triple bonds.

Aldehyde

C H, & O, C and O are always double-bonded on the end and Carbon is also single-bonded to Hydrogen

Ketone

Has carbon, hydrogen, and oxygen
Minty
Carbon and oxygen are not double-bonded on the end
One double-bonded o

Alcohol

Has carbon hydrogen and oxygen
Oxygen and Hydrogen are single-bonded together

Ester

Has carbon hydrogen and oxygen
COO in the middle
Smells sweet

Isomers

Compounds with the same formula but different structures.
Even though isomers are made from the same atoms, they have unique properties because they often form different functional groups.

Structural Isomer

Different connectivity of atoms.

Amine

Has carbon hydrogen and nitrogen
Smells fishy
Has a Nitrogen with multiple single bonds 2-3

Smells

Organic compounds smell, but 1st they must find a way into your nose
To smell them, they must evaporate (liquid to gas) or sublimation (solid to gas)

Ether

Has carbon oxygen and hydrogen
No O on the end
Has an O in the middle of two single bonds

Acid/Carboxylic Acid

Has carbon oxygen and hydrogen
Smells bad/tastes bad because of weak acids

What element goes in the middle of a dot structure?

The one that can make the most bonds, normally carbon

What do atoms in the same column have?

The same dot structure