chem ionic and metallic bonding

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Ionic Bonding Characteristics:

• Electrons transferred (localized)

• Metal + Non-Metal

• Form Giant Rigid Lattice Structure

• Electrostatic attraction

• Conductors only in liquids

• High M/P and B/P

Metallic Bonding Characteristics:

• Electrons delocalized (mobile)

• Cations in sea of electrons

• Form Giant Crystal Lattice Structure

• Mixture of metal is called an alloy

• Conductors in solids and liquids

• High M/P and B/P

Covalent Bonding Characteristics:

• Electrons shared (localized)

• Non-metal + Non-metal

• Forms individual molecules

• Good insulators (no charge)

• Low M/P and B/P

Cation:

(Metals) Positive with fewer electrons

Anion:

(Non-Metals) Negative with more electrons

Alloy:

A mixture of metals

Hydrate:

A compound that has a specific number of water molecules bound to its atoms

Polar-Covalent:

Shared unevenly

Non-Polar Covalent:

Shared evenly

The 6 Polyatomic ions are:

Nitrate →(NO3) -1

Sulfate →(SO4) -2

Phosphate →(PO4) -3

Carbonate →(CO3) -2

Ammonium →(NH4) +1

Hydroxide →(OH) -1

Rules of Sig Figs:

• leading zeros never count as sig figs even with a decimal point (Ex: 0.00415, only 415 is significant)

• trailing zeros with a decimal count (Ex: 0.38200, 38200 is significant)

• Trailing zeros without a decimal do not count (Ex: 560,000, 56 is significant)

Sig Figs: Addition and Subtraction

Round answer to the least specific decimal place

Sig Figs: Multiplication and Division

Round answer to the least amount of sig figs

Transitions Metal Exceptions that don't take Roman Numerals:

• Zinc (Zn) →+2 permanent charge

• Silver (Ag) → +1 permanent charge

• Aluminium (Al) →+3 permanent charge

Roman Numerals:

1: I

2: II

3: III

4: IV

5: V

6: VI

7: VII

8: VIII

9: IX

10: X

How to calculate Molar Mass:

(Mass of element) x Subscript + (Mass of element) x Subscript = Answer g/mol

Percent Composition:

Mass of element/Mass of compound x 100