# data[].attributes.body
The reason for the high melting and boiling temperatures is the hydrogen bonding between water molecules that causes them to stick together and to resist being pulled apart which is what happens when ice melts and water boils to become a gas.

# data[].attributes.headline
Ionic Compounds- Naming ionic compounds 

# data[].attributes.subject
Ionic Compounds- Naming ionic compounds 

# data[].attributes.body
An ionic compound is named first by its cation and then by its anion. The cation has the same name as its element. For example, K⁺¹ is called the potassium ion, just as K is called the potassium atom. The anion is named by taking the elemental name, removing the ending, and adding “ide.” or “ite”  or “ate”

# data[].attributes.body
Hard.

Form crystal lattices not molecules.

Good insulators.

High melting points/ Boiling Points.

Conduct electricity when dissolved in water or as a liquid.

Solids do not conduct electricity.

# data[].attributes.body
When writing a chemical formula, the cation comes first, followed by the anion. This is because

# data[].attributes.headline
Polarity and Dipole-Dipole Interactions 

# data[].attributes.subject
Polarity and Dipole-Dipole Interactions 

# data[].attributes.body
Molecular dipoles occur when there is an uneven spread of electrons making one side of the molecule slightly positive and the other side slightly negative. Permanent dipoles occur when molecules have very different electronegativities. One atom attracts the electrons more than the other meaning that one side is slightly negative and the other side is slightly positive. Molecules that have a permanent dipole-dipole interaction are called polar molecules.

# data[].attributes.headline
Covalent Bonding: Non- metal and non- metal 

# data[].attributes.subject
Covalent Bonding: Non- metal and non- metal 

# data[].attributes.body
Non- metals are lovers of electrons, therefore they need to gain electrons to reach stability rather than lose electrons. Covalent bonding is when two atoms share electron pair(s). This happens with non- metals only because they both need to gain more electrons to complete the octet rule.

# data[].attributes.body
a bonding pair represents the pair of electrons in the valence shell being shared in a covalent bond. Non-bonding pairs represent the valence electron pairs in an atom not being shared in the bond. #lonerz

# data[].attributes.body
Rule One: the element with the lower group is written first in the name, the element with the higher group number  goes second.
*exception: when the compound contains oxygen and a halogen, the name of the halogen is the first word in the name.

Rule Two: If both the elements are the same group, the element with the higher period number goes first.

Rule 3: the second element is the name is name as is were an anion, by adding the suffix- ide to the name of the element.

Rule 4: A prefix is used in front of each element name to indicate how many atoms of that element are present.

1-mono
2-dix
3-tri
4-tetra
5-penta
6-hexa
7-hepta
8-octo
9-nono
10-deca

*exception: if there is only one of the first element, the prefix for one is dropped.

# data[].attributes.headline
Ionic Bonding- Metal and non - metal (cation and anion)

# data[].attributes.subject
Ionic Bonding- Metal and non - metal (cation and anion)

# data[].attributes.body
An ionic bond is formed between a metal and a non-metal. Non-metals(-ve ion) are "stronger" than the metal(+ve ion) and can get electrons very easily from the metal. These two opposite ions attract each other and form the ionic bond.
Examples: Sodium chloride (NaCl), Sulfuric Acid (H₂SO₄ )

# data[].attributes.headline
Single, Double and Triple Covalent Bonds 

# data[].attributes.subject
Single, Double and Triple Covalent Bonds 

# data[].attributes.body
Covalent bonds are bonds that are between non-metal elements because they're both LOVERS of electrons and therefore resort to sharing electrons.
A double covalent bond is when there are two electron pairs are shared and a triple bond is where three electron pairs are shared

# data[].attributes.body
General properties of most metals:

Solid at room temperature (expect Mercury)

High melting point

Good heat and electricity conductors

Malleable

Ductile

Strong

Dense

Why are metals strong???
The atoms in a pure metal are tightly packed together in a lattice structure which enables the layers of metal ions slide over each other preventing the structure from shattering.which in turn makes the metals strong.

Why are metals Ductile and Malleable?
Because the metal ions slide over each other whilst the 'electron sea' glues them together.

Why are metals good heat and electricity conductors?
The outer valence electrons become delocalised so they are able to move around the structure freely between the lattice of positive metal ions.. When the metal is heated the delocalised electrons gain kinetic energy which makes them move faster and allows the transfer of energy through the metal.

# data[].attributes.body
The table shows the symbol of the ions and the charge (positive or negative)

# data[].attributes.body
Ions are formed when atoms lose or gain electrons in order to achieve the octet rule and have full outer shell.
Cations are positively charged meaning they lost electrons and anions are negatively charged meaning they gained electrons.
Eg:
- Fluorine gains 1 to become F-
- Boron loses 3 to become B3+

# data[].attributes.body
-Linear
-Bent
-Triangular Pyramid
-Trigonal Planar
-V-shape
-Tetrahedral

The reason for the shapes of the molecules, is because of the electron clouds and the electrons pushing away to get as far away from other electrons as possible

# data[].attributes.body
covalent compounds usually have low melting points and low boiling points as they have weak attraction forces between the molecules (intermolecular) which means less energy is needed to break the force of the bonding.

# data[].attributes.body
Delocalised electrons are electrons the in a metallic bond that are free to move though a whole lattice structure. The electrons in a metallic bond are known as a sea of electrons. The picture below is showing how the delocalised electrons are always moving around the elements.

# data[].attributes.body
is only between metal elements. As the metals are typically in groups 1, 2 & 3 in the periodic table, they are trying to lose the extra electrons in their valance shell to get either a full outer shell or and outer shell of 8. Since they are losing their electrons, they have  positive charge.