chemistry

• Alkali metals are highly reactive
• Ionic Bonding = one atom DONATES electrons to another atom.
• Covalent Bonding= the sharing of electrons between (2) atoms.

  (2 atoms SHARE electrons)
• Metallic Bonding = when atoms LOSE their OUTERMOST electron COMPLETELY.
• Acids have a pH less than 7
• The pH scale measures how acidic/alkaline something is. It ranges from 0-14 with 7 being neutral.
• Bases have a pH greater than 7
• Neutral substances have a pH equal to 7
• pH is measured using a pH meter or litmus paper.
• Ionic BOND- a CHEMICAL bond formed between two ions with opposite charges. (* a metal and a non-metal * )
• Group 1 = Alkali Metals
• Group 2 = Alkaline Earth Metals
• Ionic BOND is formed by the TRANSFER of ions (oppositely charged) form one to the other.
• Metals lose IONS (electrons) to form CATIONS (positive ions)
• Non- Metals GAIN IONS (electrons) to form ANIONS (negatively charged ions)
• Positive cations and Negative anions ATTRACT each other
• IONIC BONDING = a strong electrostatic FORCE OF ATTRACTION between POSITIVE CATIONS and NEGATIVE ANIONS
• IONIC BONDING - A chemical bond that forms between oppositely charged ions.
• Ionic Bonding - the forces of attraction between positive cations and negative anions
• IONIC *BONDING* properties -

  high melting and high boiling point

  insulator - doesn't conduct electricity when solid

  conducts electricity when molten/ aqueous

  usually soluble in water
• COVALENT BONDING - The sharing of pairs of electrons between nonmetal atoms.
• Covalent Bonding is when two atoms share electrons, forming a molecule.
• Covalent Bonding - two or more atoms share one or more pairs of electrons to form molecules
• Covalent Bonding Properties - low melting and boiling points (except noble gases)
• Covalent Bonding Properties - usually insoluble in water
• Covalent Bonding Properties - insulators (except graphite) - don't conduct electricity when solid
• Covalent Bonding Properties - poor conductor of heat and electricity
• Covalent bonding properties - usually not soluble in water
• Covalent Bonding Properties - some have high density
• Ionic Bonding is the attraction between oppositely charged ions.
• Ionic Bonding - electrostatic attraction between oppositely charged ions
• Ionic Bonding Properties - high melting and boiling points
• Electronegativity - Measures the tendency/ likelihood of an atom to attract electrons towards itself.
• Metals - Metals are elements on the Periodic Table that are

  1. MALLEABLE (can be hammered into thin sheets) and ductile (can be drawn into wires)/(a metal/ other material that can be hammered/pressed into a shape without breaking/cracking)
  2. Loses Electrons easily
  3. Good conductors of heat and electricity
  4. typically appear reflective. (luster)
• Non-Metals are elements that do not form positive ions in an aqueous solution.
• Nonmetal properties include being brittle, poor conductor of heat and electricity, low melting point, and dull appearance.
• Elements with similar chemical properties have similar electron configurations.
• The periodic table is organized by atomic number and electron configuration.
• The periodic table is organized by increasing atomic number.
• Periods represent different energy levels or shells around the nucleus.