Chemistry 11 exam

• What is matter?


  Anything that has mass (weight) and takes up space (volume)
• What is mass?


  A measure of the amount of matter in an object
• What is volume?


  The amount of space an object takes up
• Physical (Qualitative) properties


  Measured with 5 senses
• What is a proton?

  positively charged subatomic particle found in the nucleus

  2000x smaller than an electron
• What is a Neutron?

  a neutrally charged ion inside the nucleus with proton

  2000x smaller than an electron
• What is an electron?

  a negatively charged subatomic particle located in teh energy levels of an atom

  2000x larger than a proton and neutron
• What is atomic radius?

  the distance from the nucleus to the outermost electron

  measured in pictometers (pm)
• effective nuclear charge (Zeff)

  opposites attract electrons (-) are attracted to protons(+) in the nucleus
• atomic radius down a group

  Increases because more electron levels are added

  Electrons are negative and repell eachother increasing the atomic size
• atomic radius across a period

  Decreases- more protons are in nucleus pulling the electrons tighter together (attractive force is stronger)
• Ionic Radius


  Distance from the center of an ion's nucleus to its outermost electron
• Ionic radius from metal to cation

  always smaller than the original neutral atom be it loses a valence energy level to achieve stability
• Ionic radius from nonmetal to anion

  gains an energy level (always bigger than original neutral ion)
• Anion


  A negatively charged ion
• Ion


  An atom or group of atoms that has a positive or negative charge.
• Cation


  A positively charged ion
• Ionization energy


  The amount of energy required to remove an electron from an atom's Valence
• Ionization energy across a period

  increases as the proton# increases making the attractive pull stronger and requiring more energy to remove
• Ionization energy down a group

  decreases: more electron shielding, effective nuclear charge decreases, easier to take electrons (less attractive pull/force
• Electronegativity


  the ability of an atom to attract a bonding pair of electrons to itself
• Electronegativity across a period

  EN increases as more protons (atomic #) are added, creating a greater attractive force+bonds
• Electronegativity down a group

  Decreases because electrons are further away from nucleus
• Electron affinity


  Energy released when atoms are added
• Electron affinity across a period

  Increases as more protons are added creating a greater attractive force
• Electron affinity down a group

  decreases as distance from nucleus increases (more energy levels= further away)
• What does 'isoelectronic' mean?

  Having the same number of electrons as a noble gas
• isoelectronic' When do you add a positive charge?

  To subtract electrons
• isoelectronic' When do you add a negative charge?

  To add electrons
• ionic compound


  A compound that consists of positive and negative ions
• ionic


  Metal + nonmetal:

  Formed when one or more electrons are transferred from one atom to another
• molecular


  Non-metal +Non-metal:

  of, relating to, or consisting of molecules.
• Molecular compound


  a compound composed of molecules
• ionic compound characteristics


  have very high melting points and boiling points

  
  

  dissolve readily in water and other polar convent and are good conductors of electricity
• molecular compound characteristics


  Gas at room temp. because they have less intermolecular forces, low melting/boiling points, bad conductors because charged particles aren't moving
• Intermolecular force


  forces of attraction between molecules
• Intramolecular force


  forces that hold atoms and ions together in molecules and compounds
• Bond formed when the EN difference is larger than 1.7

  Ionic bond
• Bond formed when the EN difference is samller than 1.7

  Covalent bond (molecular)
• Non polar bonds


  covalent bonds where electrons are shared equally between atoms