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Ionic
Covalent
Metallic
Lewis & VSEPR
Intermolecular Forces
100
What factor determines whether a bond is Ionic or Covalent? What are the values for either type of bond?
What is electronegativity 0 to 1.7- covalent 1.7 or higher -ionic
100
Why do atoms form chemical bonds? What is bond length?
What is to become more stable bond length = potential energy minimim for 2 atoms sharing electrons
100
What is the model for metallic bonding? How is the strength of metallic bonding measured?
What is the Electron Sea Model. Enthalpy of Vaporization -energy needed to vaporize 1 mole of a metal
100
Draw the Lewis structure for PH3 and give its geometry.
What is trig. pyramid
100
OK, so what are Intermolecular forces and why should we care?
What is forces of attraction between molecules. We wouldn't be here without them!
200
Describe/draw the structure of an ionic compound. What is the force of attraction?
What is crystal + - + - + - cation attracted anion
200
What is the octet rule? what atoms are exceptions to the rule?
What is atoms tend to form bonds so that each atom shares or has 8 electrons in its valence shell. B -6 electrons, Be -4, P,S and others (3rd period or higher)-expanded octets (10 or 12)
200
Why are metals malleable and ductile?
What is the structure is the same in all directions. A shift in any one direction doesn't change the cation -cation interactions
200
Draw the Lewis structure for CF4 and give the geometry. Is the molecule polar? Explain
What is tetrahedral. Nonpolar -dipoles cancel out.
200
What is the strongest type of intermolecular force and what atoms are involved?
What is Hydrogen bonding, N,O,F bonded to H
300
How is the strength of an ionic bond measured? Explain.
What is lattice energy -energy released when 1 mole of an ionic crystal is formed from gaseous ions.
300
How do single, double and triple bonds differ? Order them from strongest to weakest.
What is 1,2,3 pairs of shared electrons. Triple>Double>Single
300
Explain why metals are shiny, lustrous?
What is low lying d orbitals. Metals absorb E at all different frequencies, exciting electrons into empty orbitals. The excited electrons relax back down releasing photons at all differnt frequencies/wavelengths.
300
What is resonance?
What is when a molecule cannot be represented by a single Lewis Structure.
300
What type of force is reponsible for an increase in solubility of nonpolar compounds in polar solvents?
What is Dipole -Induced dipole Solubility of Oxygen in water
400
Are Ionic compounds conductive? When?
What is in the molten state, or dissolved in water
400
How do covalent compounds differ from covalent network solids? How are they similar
Similar -nonmetals covalently bonded Differ -Covalent cmpd -single molecule Covalent Ntwk -3D array of covalently bonded atoms (ex. diamond, graphite SiO2) very different properties -mp, bp, hardness
400
What determines the strength of a metallic bonding?
What is nuclear charge (cation) and the # of electrons in the electron sea
400
How does VSEPR theory predict molecule geometry -on what basis?
What is that the electron pairs surronding a central atom will attempt to get as far apart from each other as possible (electron-electron repulsion)
400
Name the weakest of the Intermolcular Forces. What is this force dependent on?
What is London Dispersion forces dependent on the SIZE of the molecule
500
Are ionic compounds malleable? Explain.
What is Nope Shift in the crystal structure ---> cation -cation and anion-anion interactions
500
Draw the Lewis structure and predict the geometry for SeH2
What is bent
500
Describe how metallic bonding is similar to ionic bonding. How is it different?
Similar- ions are in relatively fixed 3D array, high mp, bp Differ -Metallic electrons are free to move (d orbitals) -conduct, no directionality in metals -malleable,
500
Draw the Lewis structure and predict the geometry for IF5.
What is square pyramid
500
What are hybrid orbitals and how do they relate to atomic orbitals?
What is the mixing of atomic orbitals to form hybrid orbitals # of atomic orbitals = #hybrid orbitals E of hybrid is between the atomic orbitals