MCAT Chemistry

The ___ is the basic building block of matter. An atom is composed of subatomic particles called _____, neutrons and _____. The protons and neutrons in an atom form the ____, the core of the atom.

Protons carry a single ____ charge. The ____ number of an element equals the number of protons found in an atom of that element.

____ carry no charge. Isotopes have different numbers of ____ but the same number of protons and exhibit ____ chemical properties. The ____ number of an element is equal to the total number of protons and neutrons.

^AX_z where A is the mass number and Z is the ____ number.

Electrons carry a charge equal in magnitude to but opposite in sign to that of _____. An electron has a very ____ mass. The electrons farthest from the nucleus are known as _____ electrons.

The farther the valence electrons are from the nucleus, the ____ the attractive force of the positively charged nucleus and the ____ likely the valence electrons are to be influenced by other atoms.

In a neutral atom the number of electrons is equal to the number of _____.

The first quantum theory proposes that energy emitted as electromagnetic radiation from matter comes in discrete bundles called ____.

The energy value of a quantum is: E=hf where h is Planck's constant and f or v is the ____ of the radiation.

The energy of an electron is related to its ____ radius: The smaller the radius the ____ the energy state of the electron.

At the ground state level, n=1, the electron is in its ____ energy state. At room temperature, the majority of atoms are in the ____ state, however, electrons can be excited to higher energy levels by ____ or other energy. The lifetime of the excited state is _____ and the electrons return rapidly to the ground state, emitting energy in the form of _____.

E= hc/wave length of radiation

Electrons are described as being in a state of rapid motion within regions of space around the nucleus called ____. An orbital is a representation of the ____ of finding an electron within a given region.

The Heisenberg uncertainty principle states that it is impossible to determine, with perfect accuracy, the momentum and ____ of an electron simultaneously.

The four quantum numbers are n, l, m_l, and m_s.

The values of the quantum numbers qualitatively give information about the orbitals: n about the ___, l about the ___ and m_l about the____ of the orbital

The ______ quantum number is n. The larger the integer value of n, the ____ the energy level and radius of the electron's orbit.
*The maximum number of electrons in energy level n is 2n²*

The azitmuthal(angular momentum) quantum number, l, refers to the ____ that occur within each principal energy level.

For any given n, the value of l can be any integer in the range of 0 to n-1. The four subshells corresponding to l=0,1,2 and 3 are s, p, d, and f respectively.

The maximum number of electrons that can exist in a subshell is given by the equation: 4l+2.

The greater the value of l, the greater the ____ of the subshell.

The magnetic quantum number, m_l specifies the particular ____ within a subshell where an electron is hiighly likely to be found at a given poiny in time. m_l ranges from l to -l.

Electron configuration: 2p⁴
2= ____ level
p = subshell
4= # of electrons in the _____.

Hund's rule states that within a given subshell, orbitals are filled such that there are a maximum number of ____-filled orbitals with parallel spins; electrons prefer empty orbitals to half-filled ones because a ____ energy must be overcome for two electrons carrying _____ negative charges to exist in the same orbital.

Elements in the same group have the same electronic _____ in their valence (outermost) shell and share ____ chemical properties.

Valence electrons are the electrons involved in chemical ____ and determine the chemical reactivity and ____ of the element.

From left to right across a period, electrons of the outermost (valence) shell experience an increasing amount of _____ attraction, becoming closer and ____ tightly bound to the nucleus. Going down a column the electrons become ____ tightly bound to the nucleus.

From left to right, the number of protons increases producing a greater positive charge, which means a decrease in the number of electrons, thus the atomic radius _____ from left to right. Going down a group, the atomic radius ____.

Ionization energy is the energy required to ____ an electron completely. Removing an electron requires an input of energy, which means it is an _____ reaction. The closer and more tightly bound an electron is to the nucleus, the ____ it is to remove and the ____ the ionization energy will be.

Atomic radius decreases from left to right on the periodic table and increases going down a column, thus, from left to right ionization energy ____ and down a column ionization energy _____.

Electron affinity is the willingness of an atom to ____ an additional electron. From left to right, electron affinity _____ and going down a column it ____.

Electronegativity is a measure of the attraction of an atom for ____ in a chemical bond. The greater the electronegativity of an atom, the _____ its attraction for bonding electrons. Elements with low ionization energies will have ____ electronegativities. Like ionization energy, from left to right electronegativity _____ and down a column _____.