chem_bonding Flashcards
Define valence electrons.
Valence electrons are those electrons furthest from the nucleus (i.e. in the outer shell) - which are typically involved in covalent bonding.
Describe a reliable method to determine the number of valence electrons for an element.
The number of valence electrons can be determined by refering to which main-group column the element is found in. For example nitrogen is found in main-group 5 and therefore nitrogen has 5 valence electrons. These are the electrons described by the 2s22p3 electron configuration.
List the steps in drawing a Lewis structure.
The steps are
- Count the total number of valence electrons (add 1 for a negative charge, subtract 1 for a postive charge).
- Draw a molecular skeleton generally with the least electronegative element in the center and joining each atom with a dashed line.
- Place enough electrons to give each element an octet (hydrogen only needs a duplet).
- If Step 3 uses too many electrons- take away the excess electrons and make the appropriate double bond or triple bonds. If Step 3 uses too few electrons, add the required number of electrons to the central atom.
- Assign formal charges to all atoms.
- Draw all necessary resonance forms.
Define formal charge.
Formal charge is an apparent charge which results if an atom “owns” more or less electrons than its normal count of valence electrons. All lone pairs plus 1/2 of the shared pairs are “owned”. Formal charge is therefore calculated by subtracting the number of electrons “owned” from the normal count of valence electrons.
Define resonance (structure) form.
Resonance forms are two or more Lewis structures drawn (seperated by double headed arrows) to indicate the existance of delocalized electrons. Delocalized electrons are the result of pi electrons being shared between three or more atoms (instead of just two atoms).
Explain VSEPR theory.
Valence Shell Electron Pair Repulsion (VSEPR) theory predicts that electron pairs about a central atom will arrange themselves so as to minimize repulsion. Electron pairs include both bonding and lone pairs.
Define steric number (SN).
Steric number (SN) is a parameter about a central atom which accounts for the number of regions of electron density. It is calculated by: number of sigma bonds + number of lone pairs.
Compare and contrast electronic versus molecular geometry.
Electronic geometry describes the arrangement of the electron pairs about the central atom. There are five basic geometries: linear, trigonal planar, tetrahedral, trigonal bipyramidal and octahedral. The electronic geometry is essentially determined by the central atom’s steric number (SN).
Molecular geometry describes the arrangement of atoms around a central atom. Molecular geometry is essentially determined by the electronic geometry.
Molecular geometry is identical to electronic geometry when there are no lone pairs of electrons. For example the electronic and molecular geometry of CH4 is tetrahedral (SN = 4, AX4-type molecule). By contrast the electronic geometry of NH3 is tetrahedral (SN = 4), but the electronic geometry is trigonal pyramidal (AX3E-type molecule). In this case NH3 has one lone pair of electrons.
Give the name of the electronic and molecular geometries for an AX3E2-type molecule.
AX3E2-type molecule has an electronic geometry essentially the same as an AX5-type molecule - that is trigonal bipyramidal. Its molecular geometry is T-shaped.
Give the name of the electronic and molecular geometries for an AX4E2-type molecule.
AX4E2-type molecule has an electronic geometry essentially the same as an AX6-type molecule - that is octahedral. Its molecular geometry is square planar.
Give the name of the electronic and molecular geometries for an AX4E-type molecule.
AX4E-type molecule has an electronic geometry essentially the same as an AX5-type molecule - that is trigonal bipyramidal. Its molecular geometry is see saw.
Give the name of the electronic and molecular geometries for an AX5E-type molecule.
AX5E-type molecule has an electronic geometry essentially the same as an AX6-type molecule - that is Octahedral. Its molecular geometry is square pyramidal.
Give the name of the electronic and molecular geometries for an AX2E3-type molecule.
AX2E3-type molecule has an electronic geometry essentially the same as an AX5-type molecule - that is trigonal bipyramidal. Its molecular geometry is linear.
When does electronic geometry = molecular geometry?
Molecular geometry is identical to electronic geometry when there are no lone pairs of electrons. For example the electronic and molecular geometry of CH4 is tetrahedral (SN = 4, AX4-type molecule). By contrast the electronic geometry of NH3 is tetrahedral (SN = 4), but the electronic geometry is trigonal pyramidal (AX3E-type molecule). In this case NH3 has one lone pair of electrons.
Define electronegativity.
Electronegativity is the attraction the nucleus has for a shared pair of electrons.