152 cards
Those electrons in the valence shell that are not involved in covalent bonds are ____ electrons.
The number of dots in Lewis Structure notation comes from ____ numbers.
The difference between the ____ is the formal charge.
The difference between the number of electrons assigned to an atom in a Lewis structure and the number of electrons normally found in that…
To equation for formal charge is:
The charge of an ion or compound is equal to ____.
A less formal way to calculate formal charge is with the formula: Formal charge = ____.
____s overestimate the effect of electronegativity differences.
Formal charge ____ the effect of electronegativity differences.
Resonance structures allows for greater stability, ____ electrons and charges over what is known as a π (pi) system.
Resonance structures allows for greater stability, delocalizing electrons and charges over ____.
____ structures allows for greater stability, delocalizing electrons and charges over what is known as a π (pi) system.
The nature of the bonds within the actual compound is a ____ of the possible resonance structures.
Actual structure of the compound with resonance structures is called ____.
In general, the more ____ the structure, the more it contributes to the character of the resonance hybrid.
A Lewis structure with ____ formal charges.
A Lewis structure with ____ separation of opposite charges.
A Lewis structure in which negative formal charges are placed on ____ electronegative atoms.
Nonmetals ____ so as to achieve a stable octet.
Metals ____ so as to achieve a stable octet
____ uses Lewis dot structures to predict the molecular geometry of covalently bonded molecules.
VSEPR theory uses Lewis dot structures to predict ____ of covalently bonded molecules.
The following steps are used to predict the geometrical structure of a molecule using the VSEPR theory: 1. ____.
____ geometry describes the spatial arrangement of all pairs of electrons around the central atom, including both the bonding and the lone…
Electronic geometry describes ____.
____ geometry describes the spatial arrangement of only the bonding pairs of electrons.
Molecular geometry describes ____.
____, which is the number of atoms that surround and are bonded to a central atom.
Tetrahedral electronic geometry, for example, is associated with an ideal bond angle of ____.
Nonbonding electron pairs are able to exert more ____ than bonding electron pairs because these electrons reside closer to the nucleus.
____ electron pairs because these electrons reside closer to the nucleus.
Tetrahedral electronic geometry, for example, is associated with an ideal bond angle of 109.5°; however, the angle in ammonia is closer to…
The presence of bond dipoles results in a molecular dipole. ____
When the molecular geometry is arranged such that the bond dipoles do not cancel each other out, the molecule will have a ____.
When the molecular geometry is arranged such that the bond dipoles do ____, the molecule will have a net dipole moment and will therefore b…
The ____ quantum number, n, indicates the average energy level of the shell.
The principal quantum number, ____, indicates the average energy level of the shell.
The principal quantum number, n, indicates ____.
The ____ quantum number, l, describes the subshells within each principal energy level.
The azimuthal quantum number, ____, describes the subshells within each principal energy level.
The azimuthal quantum number, l, describes ____.
When l = ____, this indicates the s subshell, which has one orbital that is spherical in shape.
When l = 0, this indicates the ____ subshell, which has one orbital that is spherical in shape.
When l = 0, this indicates the s subshell, which has o____ in shape.
When l = ____, this indicates the p subshell, which has three orbitals shaped like barbells along the x -, y -, and z -axes at right angles…
When l = 1, this indicates the ____ subshell, which has three orbitals shaped like barbells along the x -, y -, and z -axes at right angles…
When l = 1, this indicates the p subshell, which has ____ along the x -, y -, and z -axes at right angles to each other.
____ analysis of the wave functions of the orbitals is used to determine and assign plus and minus signs to each lobe of the p -orbitals.
Mathematical analysis of the wave functions of the orbitals is used to determine and assign ____ to each lobe of the p -orbitals.
When two atoms bond to form a compound, the atomic orbitals interact to form a ____ .
____ describes the probability of finding the bonding electrons in a given space.
Molecular orbital describes the probability of finding the ____ electrons in a given space.
Molecular orbitals are obtained by combining the ____ of the atomic orbitals.
Qualitatively, the overlap of two atomic orbitals describes ____.
If the signs of the two atomic orbitals are the same, ____ forms.
If the signs of the two atomic orbitals are ____, a bonding orbital forms.
If the signs of the two atomic orbitals are different, ____ forms.
If the signs of the two atomic orbitals are ____, an antibonding orbital forms.
When orbitals overlap head-to-head, the resulting bond is ____.
When orbitals overlap ____, the resulting bond is a sigma ( σ ) bond .