Chemistry test bond theories Exam Questions And Answers

How does adding an atom affect the position of existing atoms or lone pairs? - ANS pushes them away from the newly added atom How does adding a lone pair affect the position of existing atoms or lone pairs? - ANS same as adding an atom, pushes them away from the newly added Are adding atoms/ lone pairs similar? - ANS yes, because all electrons repel each other How do the electrons in bonds (bonding domains) differ from lone pairs( non-bonding domains)? - ANS bonded electrons are shared between 2 elements, where lone pairs belong only to the atom they are attached to Can you force the atoms into new configurations by pushing atoms around? What does this suggest about configurations in real models? - ANS no, as soon as you push an atom, other move to keep the same distance between bonds What happens to the bond angle when you add or remove an electron domain? - ANS decreases What is molecular geometry? - ANS 3d shape based on # of electron areas around the center element line= - ANS in the plane of the paper wedge= - ANS coming forward, in front of the plane of the paper dash= - ANS going backward, behind the plane of the paper What is the difference between electron geometry and molecule geometry - ANS electron geometry is the sub group of shape that occur when a lone pair of electron is present on center, while molecule geometry is the overall name/shape based on number of areas around center Orbital: the region in space where there is a high _________ of finding the electrons? - ANS probability x,y, and z give the _________ of orbitals? - ANS orientation the bond between 2 atoms is the result of the overlap of their atomic orbitals? - ANS Molecular bond theory the increase in the electron density lies directly between two nuclei - ANS sigma bonds The increase in the electron density lies above and below the axis, connecting the two nuclei? - ANS pi bonds VSEPR stands for? - ANS valence shell electron pair repulsion _______ pairs repel more than ______ pairs. - ANS lone/ bonded This caused the bond angle to be ______ than it would be if no ______ pairs were present. - ANS less/lone 4 atoms, 0 LP? bond angle? - ANS tetrahedral/ 109.5 3 atoms, 1 LP? bond angle? - ANS tetrahedral trigonal pyramidal/ 109.5 2 atoms, 2 LP? bond angle? - ANS tetrahedral bent/ 109.5 1 atom, 3 LP? bond angle? - ANS linear/ 180