Lecture 3 Flashcards
What is an electron orbital?
a 3D space where an electron is found 90% of the time
How many electrons can occupy each orbital?
2
What is the definition of energy?
the capacity to cause change
What is potential energy?
the energy that matter has because of its location or structure
How do the electrons in an atom differ?
By their amount of potential energy
What is an electrons state of potential energy called?
energy level or electron shell
What are valence electrons?
electrons in the outermost shell (valence shell)
What influences the chemical behavior of an element?
valence electrons
How do electrons close to the nucleus behave?
they tend to stay there and they are typically hard to lose (oxidze)
What does it mean for something to oxidize?
It loses electrons
What does it mean for an element to be inert?
It has a full valence shell
What effect do unpaired electrons have on an atom?
They make atoms more reactive
How is the chemical behavior of an atom determined?
By the distribution of electrons in the electron shell
What type of bond holds together shared valence electrons with other atoms?
Chemical bonds
What are the types of covalent bonds?
polar and nonpolar
What are the types of noncovalent bonds?
Ionic, hydrogen bonds, Van der Waals, Hydrophobic interactions (not really a bond)
What is a covalent bond?
The sharing of a pair of valence electrons by two atoms
Describe the strength of covalent bonds.
strong and contain stored energy
What is a nonpolar covalent bond?
atoms share the electron equally
What is a polar covalent bond?
one atom is more electronegative, and the atoms do not share the electron equally
What does unequal sharing of electrons result in?
a partial charge for each atom or molecule
What is electronegativity?
an atoms attraction for the electrons in a covalent bond
How does electronegativity affect an atom?
The more electronegative an atom is, the more strongly it pulls shared electrons toward itself
What bond form most cell molecules?
covalent
