Atomic Structures PDF

Atomic Structures Remember: Two Primary parts of an Atom: Atomic number - it is the Nucleus – Centrally Located number if protons Orbital shell – outside the nucleus Atomic mass - mass of the...

Atomic Structures Remember: Two Primary parts of an Atom: Atomic number - it is the Nucleus – Centrally Located number if protons Orbital shell – outside the nucleus Atomic mass - mass of the particle relative to the atom Fundamental / Subatomic Particles Atomic number indicates the number of protons 3 constituents of an atom: Electron Neutrons - consider to be the most Proton unstable (discovered by James Neutrons Chadwick) Protons and neutron are made From the "neutral" meaning it of Quarks bounded by Gluons has not charged Protons + Neutrons = Nucleons Location Nucleus (Constituent of the Nucleus) Nucleon - collective term in the Electrons are mode of Leptons combined number of protons and Gluons and neutrons. Fundamental Particles Protons - served as the identity / or the most important of the atoms (discovered Earnest Rutherford) Each proton carries 1 positive charge (discovered by Eugene Goldstein) location nucleus Electrons - Lightest, the movable SAP To determine how many electrons are (discovered by J.J Thompson) present in a shell Use the formula: Found in the orbital shell or extranuclear 2(𝑛)2 Where n is the shell number of 2000 times much lighter than the principal quantum number protons and neutrons In an stable atom the number OCTET Rule of electrons is equals to the States that the outer most shell number of protons (valence shell) of an atom can only handle eight electrons. Nucleus Exception to octet rule: Small dense center of an atom If the atom only has a single as described by Earnest shell (k-shell), the k-shell can Rutherford only handle maximum of 2 electrons It is positively charged The reason why nucleus is Remember: positively charged is because the inside of the nucleus is The closer the electron the positively charged and no nucleus, the higher the electron charge binding energy (attractive energy between electron and nucleus) Electron Arrangement According to Neils Bohr the Law of electrostatic - opposite electrons is arranged in a charges attracts, same charges systematic manner. repel  The outermost shell of an atom Law of conservation of energy (Valence shell can only contain Energy cannot be created nor no more than 8 electron called destroyed OCTET Rule. Energy is just converted from Electron Binding Energy one form to another The strength of attachment of an electron to the nucleus; also Excitation the energy required to remove Is a process where energy of an electron from its shell radiation is absorbed by the particle making it in an exiting The closer the electron to the state (metastable state - nucleus, the Stronger the abnormal state) Electron Binding Energy The farther electron, the lower Atomic Numenclature the EBE Atomic Number Number of protons The larger an Atom, the greater (identification) its EBE, the harder it is to be ionized Atomic Mass Number Number of Nucleons (Protons + Ionization Neutrons) A process of removing / adding Chemical Symbol of electrons to an atom. The alphabetical abbreviation of the element Ionization can only happen if Valence State the energy if the incident Positive Valence: less than 4 radiation is equal or higher than valance electron = conductors the EBE (Electron Binding Negative Valence: More than 4 Energy) valence electron = insulators  Nuclear Families Note: The removed electron and the Isotopes remaining atom is now called an Ion Pair Atoms with same proton number or atomic number Important Terms Isobar Matter – anything that occupy space Atoms with same Nucleon and has mass number Energy – characterized by lack of Isotones occupied space, no mass, no charge Atoms with the same number of Mass – smallest particle of compound neutron and is a combination of an atom Isomer Compound – quantity of one type of Atoms with the same everything molecule Atoms with different energy Element – the pure substance state called metastable composed the same identical atoms Ionization of Atoms Ion Bonding An atom with an extra or Covalent bonds – sharing of electrons lacking electron, atom with to form a molecule charge Ionic Bonds – Occurs with ions and it Ca+ions – Lacks An Cation is the attraction of atoms due to their Positive Ions Electron electric charges. Anions – Excess in Anion Negative Ion Electron Ion – pair – the resultant of Ionization