ACS Gen Chem 1 Exam Study Guide.
Ion
A species of an element in which the number of electrons does not equal the number of protons.
Isotope
Each isotope of an atom has a different number of neutrons.
Isoelectric
Two atoms with the same charge.
Isotopic
Two atoms with the same number of neutrons.
Transition Metal Orbitals
The 4s orbital is filled before the 3d orbital, but listed after.
Paramagnetic
Atoms that possess a permanent magnetic charge due to the presence of unpaired electrons.
Electropositive
Tending to lose electrons and form positive ions.
Tetrahedral Bond Angle
109.5°
Resonance Structures
Two equally correct arrangements of one molecule's electrons; generally the molecule exists as
an average of the two.
Polar Molecule
A molecule that is mostly positive on one side and mostly negative on the other.
sp³ Orbital
An orbital composed of one s orbital and three p orbitals; can hold eight total electrons.
Tetrahedral.
Trigonal Planar
The way that three objects will arrange themselves around a central atom. Non-polar.
Free Radicals
Compounds with an odd number of electrons in their Lewis Structure. Eg. NO₂
Incomplete Octets
Occur in elements that can form stable bonds with less than eight electrons. Eg. BF₃
Expanded Octets
Occur in the third row of the periodic table and beyond in elements that can form stable bonds
with more than eight electrons. Eg. XeF₂
Hydrogen Bonding
When hydrogen is attracted to electronegative atoms.
Sigma Bonding
Formed by head-on overlapping between orbitals.
Coordinate Covalent Bonding
Ion
A species of an element in which the number of electrons does not equal the number of protons.
Isotope
Each isotope of an atom has a different number of neutrons.
Isoelectric
Two atoms with the same charge.
Isotopic
Two atoms with the same number of neutrons.
Transition Metal Orbitals
The 4s orbital is filled before the 3d orbital, but listed after.
Paramagnetic
Atoms that possess a permanent magnetic charge due to the presence of unpaired electrons.
Electropositive
Tending to lose electrons and form positive ions.
Tetrahedral Bond Angle
109.5°
Resonance Structures
Two equally correct arrangements of one molecule's electrons; generally the molecule exists as
an average of the two.
Polar Molecule
A molecule that is mostly positive on one side and mostly negative on the other.
sp³ Orbital
An orbital composed of one s orbital and three p orbitals; can hold eight total electrons.
Tetrahedral.
Trigonal Planar
The way that three objects will arrange themselves around a central atom. Non-polar.
Free Radicals
Compounds with an odd number of electrons in their Lewis Structure. Eg. NO₂
Incomplete Octets
Occur in elements that can form stable bonds with less than eight electrons. Eg. BF₃
Expanded Octets
Occur in the third row of the periodic table and beyond in elements that can form stable bonds
with more than eight electrons. Eg. XeF₂
Hydrogen Bonding
When hydrogen is attracted to electronegative atoms.
Sigma Bonding
Formed by head-on overlapping between orbitals.
Coordinate Covalent Bonding
