________: the only atoms that have their outermost shells filled with electrons; unreactive.
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Sodium
________ becomes a cation as it lost 1 electron, and chlorine becomes an anion because it gained 1 electron.
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Heisenberg
________ uncertainty principle: the uncertainty in knowing the locations of electrons at a given moment.
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Sp
________ hybridized orbitals: 2 hybridized orbitals, which are the s orbital and one of the p orbitals, and the other two remaining p orbitals remain unchanged; for atoms with 2 bonds; 180° bond angle.
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VSEPR theory
________: stands for valence shell electron pair repulsion; predicts the approximate geometry of bonds around an atom.
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Ionic bond
________: when the electronegativity difference is very large; greater than 2.
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Octet rule
________: the desire of atoms to have filled electron shells.
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Electrons
________ are equally shared between the 2 atoms.
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Polar covalent bond
________: if the electronegativity difference is smaller; between 0 and 2.
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covalent bond
Purely ________: if the electronegativity difference is 0.
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Pz
________: an orbital that points in the z direction.
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Anion
________: an atom with more electrons than the number of protons in its nucleus.
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Aufbau chart
The ________ is helpful for remembering which orbitals to fill first.
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Orbital
________: status the actual location in space of where the electron resides.
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Sp3
________ hybridized orbitals: 4 hybridized orbitals, which are the s orbital and three p orbitals; for atoms with 4 bonds; 109.5° bond angle.
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Ion
________: an atom that has more or fewer electrons than the amount of protons.
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hydrogen atoms
Because both ________ need 1 electron to fill its shell, they share their electrons equally (instead of grabbing an electron from each other)
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Py
________: an orbital that points in the y direction.
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Electronegativity
________: tendency of an atom to attract electrons towards itself.
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Px
________: an orbital that points in the x direction.
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Cation
________: an atom with fewer electrons than the number of protons in its nucleus.
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BeH2
For ________, the beryllium (Be) has two substituents (two identical H atoms), so its sp hybridized.
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Attraction
________ between sodium cation and chlorine anion in sodium chlorine is an ionic bond.
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Chlorine
________ is an atom in the second- to- last column of the periodic table and has 7 valence electrons.
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Carbon
________ (C), hydrogen (H), oxygen (O), and nitrogen (N) are the most prominent elements in organic compounds.
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Pi
________ (π): bonds where orbital overlap occurs above and below the nuclei, and not directly between them.
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Problem solving
________: Predicting bond dipole moments.
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negative charge
Because electrons spend most of the time around chlorine, chlorine gets a partially ________.
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positive charge
Because electrons spend less time around hydrogen, hydrogen gets a partially ________.
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Dipole moment
________: separation of charge in the bond because the more electronegative atom "bullies "most of the bonding electrons away from the less electronegative atom.
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net dipole moment
The ________ is zero because the oxygens are pulling in equal and opposite directions; therefore, they cancel each other out.
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Sigma
________ (σ): bonds in which orbital overlap occurs between the two bonding nuclei.
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Orbitals
________: electron shells are further subdivided into these; they are the actual location in which an electron can be found.
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Hunds rule
________: the electrons should go into different orbitals with the same spin, instead of pairing up into a single orbital with the opposite spin.
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lowest energy
First Shell: closest to the nucleus of the atom, has the ________, and can hold up to 2 electrons.
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Shell
________: indicates the energy level of a certain electron; a full shell will be spherical in shape.
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Dipole vector
________: a distinct arrow that is used to show the direction of the dipole moment, or separation of charge.
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Inorganic compounds
________: non- carbon- containing compounds.
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lone pairs
Because electrons repel each other, bonds and ________ (non- bonding electron pairs) around an atom want to be as far away from each other as possible.
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Electrons
________ are shared, but not equally between the atoms.
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Orbital
________: Apartment where the electron resides.
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Ionic bonds
________ are usually found in inorganic compounds.
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Covalent bonds
________ are found in organic compounds.
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Sodium
________ is an atom in the first column of the periodic table and has 1 valence electron.
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hydrogen atom
A(n) ________ has 1 electron, so it needs another 1 to fill its shell.
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Electrons
________ in atoms are under house arrest.
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Electrons
________ repel each other and want to be as far away from each other as possible.
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Electrons
________: they are located in the shells surrounding the nucleus, not in the nucleus itself.
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Electron House Arrest
Shells and Orbitals
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Protons
number of protons cannot be changed without changing the identity of the atom itself; if the number of protons change, it becomes a different element
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Ion
an atom that has more or fewer electrons than the amount of protons
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Anion
an atom with more electrons than the number of protons in its nucleus
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Cation
an atom with fewer electrons than the number of protons in its nucleus
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Electrons
they are located in the shells surrounding the nucleus, not in the nucleus itself
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First Shell
closest to the nucleus of the atom, has the lowest energy, and can hold up to 2 electrons
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Second Shell
higher in energy, farther away from the nucleus, and can hold up to eight electrons
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Third Shell
higher in energy than the first and second shells, even farther away from the nucleus, and can hold up to 18 electrons
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Note
there are other higher shells, but they are not dealt with in organic chemistry
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Electron apartments
Orbitals
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Orbitals
electron shells are further subdivided into these; they are the actual location in which an electron can be found
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Shell
indicates the energy level of a certain electron; a full shell will be spherical in shape
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Orbital
status the actual location in space of where the electron resides
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Electron Shell
Floor in the apartment complex (energy level)
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Orbital
Apartment where the electron resides
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Heisenberg uncertainty principle
the uncertainty in knowing the locations of electrons at a given moment
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s orbital
spherical in shape
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p orbital
shaped like a dumbbell
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1s orbital
spherically symmetric, holds 2 electrons, only orbital in the first shell
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Second Shell
contains both s and p orbitals, holds up to 8 electrons
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2s orbital
spherical shape like 1s orbital, but larger and higher in energy
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2p level
consists of 3 individual p orbitals
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Px
an orbital that points in the x direction
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Py
an orbital that points in the y direction
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Pz
an orbital that points in the z direction
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Electron instruction manual
Electron configuration
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Ground-state electron configuration
list of orbitals occupied by electrons in a particular atom
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Hunds rule
the electrons should go into different orbitals with the same spin, instead of pairing up into a single orbital with the opposite spin
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Example
Carbons electron configuration is 1s^2 2s^2 2px^1 2py^1 2pz^0 (not 1s^2 2s^2 2px^2 2py^0 2pz^0, which violates Hunds rule)
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Atom Marriage
Bonding
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Noble gases
the only atoms that have their outermost shells filled with electrons; unreactive
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Octet rule
the desire of atoms to have filled electron shells
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Valence electrons
electrons in the outermost shell of an atom; most important for bonding
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Core electrons
electrons in the inner shells; dont participate in bonding
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To Share or Not to Share
Ionic and Covalent Bonding
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Ionic Bonding
two electrons in a bond are not shared between the bonding atoms
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Covalent Bonding
two electrons in a bond are shared between the two bonding atoms
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Example of covalent bonding
hydrogen gas (H2)
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Electronegativity
tendency of an atom to attract electrons towards itself
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Ionic bond
when the electronegativity difference is very large; greater than 2
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Polar covalent bond
if the electronegativity difference is smaller; between 0 and 2
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Purely covalent bond
if the electronegativity difference is 0
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Inorganic compounds
non-carbon-containing compounds
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Separating Charge
Dipole Moments
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Dipole moment
separation of charge in the bond because the more electronegative atom "bullies" most of the bonding electrons away from the less electronegative atom
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For example
in hydrochloric acid (HCl), chlorine is the more electronegative atom of the two, so the electrons between hydrogen and chlorine are "hogged" mostly by chlorine
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Dipole vector
a distinct arrow that is used to show the direction of the dipole moment, or separation of charge
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Problem solving
Predicting bond dipole moments
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Problem Solving
Predicting molecule dipole moments
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VSEPR theory
stands for valence shell electron pair repulsion; predicts the approximate geometry of bonds around an atom
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