CHEM 135 EXAM 1
• Coulomb's Law: bigger charges means stronger bonds and the closer the bonds the
stronger the bonds. The strength of the interaction increases as the sizeof the charges increase.
• Coulomb's Law - Like Charges: potential energy is positive and decreases asthe particles
get farther apart. Far apart = more favorable
• Coulomb's Law - Opposite Charges: Potential energy is negative and be- comes more
negative as the particles get closer together. Closer together = morefavorable
• Electrons in multielectron atoms feel two forces:: attraction from positivecharge in the
nucleus and repulsion from other electrons
• Shielding: the attraction between an electron and the nucleus in any atom withmore than
one electron shell
• Effective Nuclear Charge: the positive charge that an electron experiencesfrom the
nucleus, equal to the nuclear charge but reduced by any shielding or screening from any
intervening electron distribution
• Effective Nuclear Charge Equation: Z is # of protons in nucleus, S is # ofshielding
electrons
• Penetration: If an electrons can penetrate closer to the nucleus, it will experi-ence more of
a nuclear charge, resulting in lower E (energy).
• Abbreviated Electron Configuration: shorthand notation describing the distri-bution of
electrons among the energy levels of an atom using [Noble Gases]
• Core Electrons: The electrons in the inner shells of an atom; these electronsare not
involved in forming bonds.
• Valence Electrons: The electrons in the outermost shell (main energy level) ofan atom;
these are the electrons involved in forming bonds.
• Transition Metals (Cu, Ag, Zn, Cd): Exhibit different trends concerning electron
configurations
• Electron configuration of Cu (Copper): [Ar]4s1 3d10
• Electron configuration of Ag (Silver): [Kr]5s1 4d10
• Electron configuration of Zn (Zinc): [Ar]4s2 3d10
• Electron configuration of Cd (Cadmium): [Kr]5s2 4d10
• Noble Gases Electron Config. and Properties: 8 valence electrons means fullouter quantum
levels; particularly unreactive and stable
• Halogens Electron Config. and Properties: one electron short of noble gasconfig. (ns2 np5
config.); tend to gain one electron to form a 1- ion
, • Alkali Electron Config. and Properties: one electron beyond noble gas config;tend to lose
one electron to form a 1+ ion
• Alkaline Earth Metals Electron Config. and Properties: two electrons beyondnoble gas
config; tend to lose two electrons to form a 2+ ion
• Elements that form ions with predicable charges:: Li+, Na+, K+, Rb+, Cs+,Mg2+, Ca2+,
Sr2+, Ba2+, Al3+, N3-, O2-, S2-, Se2-, Te2-, F-, Cl-, Br-, I-
• Metals tend to form...?: cations (lose electrons, positively charged)
• Nonmetals tend to form...?: anions (gain electrons, negatively charged)
• Covalent Radius: half of the distance between nuclei for two atoms covalentlybonded
together
• Van der Walls Radius: the radius of an imaginary hard sphere representing thedistance of
closest approach for another atom
• Atomic Radii: Half the distance between the nuclei of identical atoms that arebonded
together
• Atomic Radii for Anions: anions are larger in radius than their correspondingatoms
• Atomic Radii for Cations: cations are smaller in radius than their correspondingatoms
• Ions in the same group have the same..?: charge
• Larger positive charge = ?: smaller cation
• Larger negative charge = ?: larger anion
• Ionization Energy (IE): the energy required to remove one electron from aneutral atom of
an element
• Organic Compounds: Compounds that contain carbon
• Functional Groups: the components of organic molecules that are most com-monly
involved in chemical reactions
1. Mega (M): multiplier of 1,000,000
2. kilo (k): multiplier of 1,000
3. Deci (dm/d): multiplier of 0.1
4. centi (c): multiplier of 0.01
5. milli (m): multiplier of 0.001
6. micro (¼
): multiplier of 0.000000001 (10^-9)
• n: principal quantum number. determines the overall size and energy of an orbital,possible
values: any number greater than or equal to 0
• Coulomb's Law: bigger charges means stronger bonds and the closer the bonds the
stronger the bonds. The strength of the interaction increases as the sizeof the charges increase.
• Coulomb's Law - Like Charges: potential energy is positive and decreases asthe particles
get farther apart. Far apart = more favorable
• Coulomb's Law - Opposite Charges: Potential energy is negative and be- comes more
negative as the particles get closer together. Closer together = morefavorable
• Electrons in multielectron atoms feel two forces:: attraction from positivecharge in the
nucleus and repulsion from other electrons
• Shielding: the attraction between an electron and the nucleus in any atom withmore than
one electron shell
• Effective Nuclear Charge: the positive charge that an electron experiencesfrom the
nucleus, equal to the nuclear charge but reduced by any shielding or screening from any
intervening electron distribution
• Effective Nuclear Charge Equation: Z is # of protons in nucleus, S is # ofshielding
electrons
• Penetration: If an electrons can penetrate closer to the nucleus, it will experi-ence more of
a nuclear charge, resulting in lower E (energy).
• Abbreviated Electron Configuration: shorthand notation describing the distri-bution of
electrons among the energy levels of an atom using [Noble Gases]
• Core Electrons: The electrons in the inner shells of an atom; these electronsare not
involved in forming bonds.
• Valence Electrons: The electrons in the outermost shell (main energy level) ofan atom;
these are the electrons involved in forming bonds.
• Transition Metals (Cu, Ag, Zn, Cd): Exhibit different trends concerning electron
configurations
• Electron configuration of Cu (Copper): [Ar]4s1 3d10
• Electron configuration of Ag (Silver): [Kr]5s1 4d10
• Electron configuration of Zn (Zinc): [Ar]4s2 3d10
• Electron configuration of Cd (Cadmium): [Kr]5s2 4d10
• Noble Gases Electron Config. and Properties: 8 valence electrons means fullouter quantum
levels; particularly unreactive and stable
• Halogens Electron Config. and Properties: one electron short of noble gasconfig. (ns2 np5
config.); tend to gain one electron to form a 1- ion
, • Alkali Electron Config. and Properties: one electron beyond noble gas config;tend to lose
one electron to form a 1+ ion
• Alkaline Earth Metals Electron Config. and Properties: two electrons beyondnoble gas
config; tend to lose two electrons to form a 2+ ion
• Elements that form ions with predicable charges:: Li+, Na+, K+, Rb+, Cs+,Mg2+, Ca2+,
Sr2+, Ba2+, Al3+, N3-, O2-, S2-, Se2-, Te2-, F-, Cl-, Br-, I-
• Metals tend to form...?: cations (lose electrons, positively charged)
• Nonmetals tend to form...?: anions (gain electrons, negatively charged)
• Covalent Radius: half of the distance between nuclei for two atoms covalentlybonded
together
• Van der Walls Radius: the radius of an imaginary hard sphere representing thedistance of
closest approach for another atom
• Atomic Radii: Half the distance between the nuclei of identical atoms that arebonded
together
• Atomic Radii for Anions: anions are larger in radius than their correspondingatoms
• Atomic Radii for Cations: cations are smaller in radius than their correspondingatoms
• Ions in the same group have the same..?: charge
• Larger positive charge = ?: smaller cation
• Larger negative charge = ?: larger anion
• Ionization Energy (IE): the energy required to remove one electron from aneutral atom of
an element
• Organic Compounds: Compounds that contain carbon
• Functional Groups: the components of organic molecules that are most com-monly
involved in chemical reactions
1. Mega (M): multiplier of 1,000,000
2. kilo (k): multiplier of 1,000
3. Deci (dm/d): multiplier of 0.1
4. centi (c): multiplier of 0.01
5. milli (m): multiplier of 0.001
6. micro (¼
): multiplier of 0.000000001 (10^-9)
• n: principal quantum number. determines the overall size and energy of an orbital,possible
values: any number greater than or equal to 0
