Chapter 1- Atomic structure and chemical bonding Flashcards
A subatomic particle, symbol p or p+, with a positive electric charge of +1 elementary charge and a mass slightly less than that of a neutron.
Proton
A subatomic particle, symbol n or n0, with no net electric charge and a mass slightly larger than that of a proton.
Neutron
It plays as an essential role in numerous physical phenomena, such as electricity, magnetism, chemistry and thermal conductivity, and they also participate in gravitational, electromagnetic and weak interactions.
Electron
It represents the number of protons in the nucleus of an atom.
Atomic number
The total number of protons and neutrons in the nucleus of an atom.
Mass number
Atoms of the same element having the same atomic number but different atomic masses.
Isotopes
Atoms of different elements having the same mass number but different atomic numbers.
Isobars
Atoms of different elements having the same number of neutrons but differ in atomic numbers and mass numbers.
Isotones
It is the space around the nucleus in which the electron is found with a probability of 90%.
Orbital
The number of electrons in an atom are arranged in shells or ‘energy levels’ around the nucleus
Shells
Electrons are those seen in the previous noble gas and any completed transition series. They fill all the lower energy levels of an atom.
Inner (core) electrons
Are those in the highest energy level (highest n value). They spend most of their time farthest from the nucleus.
Outer electrons
Involved in forming compounds. Among the main group elements, the valence electrons are the outer electrons.
Valence electrons
It is a region of space within an electron shell that contains electrons that have the same energy.
Subshell
Describes the size of orbitals and relative distance of the electrons from the nucleus.
Principal quantum number
This refers to the shape of the orbitals.
Angular momentum quantum number
Refers to the orientation of the orbitals in space around the nucleus.
Magnetic quantum number
Describes the spin of electrons in an orbital which is opposite direction to differentiate one electron from the other in the same orbital.
Spin quantum number
The distribution of electrons in the energy levels and sublevels of an atom
Electron configuration
The number of different states of equal energy.
Degree of degeneracy or degeneracy
Electron orbitals that have the same energy levels.
Degenerate orbitals
A property of a substance to be slightly attracted to a magnetic field. It is exhibited by substances that contain one or more unpaired electrons.
Paramagnetism
A property of a substance to be slightly repelled by a magnetic field. It is exhibited by substances whose electrons are all paired.
Diamagnetism
Electrons first occupy the lowest energy orbitals available to them; only when the lower-energy orbitals are filled that they enter higher–energy orbitals.
Aufbau (building–up) principle
Only two electrons having opposite spins can occupy an orbital. The third electron will eventually be repelled.
Pauli’s exclusion principle
Electrons distribute singly before pairing.
Hund’s rule
These gases have complete e- configuration of ns2np6 except for He making them difficult to either gain or loss electrons.
Electron configuration of noble gases
The arrangement of electrons around the nucleus of an atom with lower energy levels.
The ground state
Any state other than the ground state of an atom or molecule; a state that has higher energy than the ground state.
Excited state-
An elevation in energy level above an arbitrary baseline energy state.
Excitation
The electrostatic force which holds the atoms in a compound or molecule. This results from the gain and loss of electrons, or from the sharing of electrons between atoms.
Chemical bond-
The ability of an atom to form bonds.
Valance.
States that atoms are most stable when they have a full shell of electrons in the outside electron shell.
Octet rule
It is a chemical bond resulting from the mutual attraction of oppositely charged ions.
Ionic bonding
Formed from the force of electrostatic attraction between oppositely charged ions (cations and anions).
Ionic bonding
It is an electrically charged atom of an element or group of atoms that carries an electrical charge.
Ion
It is a positively charged atom of an element. It is formed when an atom loses electron (s).
Cation
A negatively charged atom of an element. It is produced when an atom gains electron(s).
Anion
Formed when atoms share a pair of electrons to form covalent molecules.
Covalent
Bond formed when the combining atoms have a big difference in their electronegativity values, and that the sharing of the electrons is not equal.
Polar covelant bond
This type of bond is formed from the combination of atoms of the same element or atoms whose electronegativity values are very close.
Non-polar covalent bond
A type of covalent bond where the two electrons in the bond are only donated by a single atom.
Coordinate covalent bond
Shows the valence electrons in an element.
Lewis structure
States that the bond energy is inversely related to the bond length (r), and so factors which influence a bond’s strength influence its length.
Coulomb’s law
The number of electrons that an atom will lose or gain in order to get stable electronic configuration in forming ionic bond.
Electrovalency
The number of electrons that an atom can share to get a stable electronic configuration.
Covalency:
The energy required to remove an electron from a neutral atom.
Ionization potential
The energy released when an atom gains one electron to the element.
Electron affinity
A measure of the ability of an atom in a molecule to attract electrons to itself.
Electronegativity
