Please enable JavaScript.
Coggle requires JavaScript to display documents.
Final Exam (The electrons in each orbital are in the S level is 2…
Final Exam
The electrons in each orbital are in the S level is 2 electrons,p orbital is 6 electrons,d orbital is 10 electrons, and a f orbital is 14 electrons
Cations are positive ion and they will lose an electron while anion is negative and they will gain a electron
Group 1: Lose electron, gain one electron group 2 will lose two electrons but then gain two group 3 will lose 3 electrons, group 6 will gain 2 electrons but will lose two, group 7 will gain 1 electron, then will lose 1, but group 8 will gain or lose None
Valence Electrons: Highest energy level
When atoms give up electrons they are negative, but when they gain electrons, they are positive
Ionic Compounds: Metal/Non metal : they will have high melting and boiling points
In ionic compounds and molecular compounds, the second element will always end with IDE
Octet Rule: Rule of eight
Molecular Compound is non metal/ non metal
Poly atomic ions: Are when two atoms are convalescent bonded
the seven diatomic molecules are FLUORINE, HYDROGEN, OXYGEN(DOUBLE), BROMINE, CHLORINE, IODINE, NITROGEN( TRIPLE)
Coordinate Covalent Bond: When atoms contribute to both electrons to fill the share
Valence Shell Electron Pair Repulsion: L dictates of the molecule
Polar bonds: 2 non metals that have different electronnegtivity
Single Covalent Bond: 2 Double Covalent bond is 4 Triple Covalent bond is 6
10 prefixes: MONO,DIA,TRI,TETRA,PENTA,HEXA, HEPT, OCTA, NONA, DECA.
Examples of prefixes: NCl3, Nitrogen Trichloride
Binary Molecular Compounds Examples or opposite of above Phosphorus pentchloride: PhCl5
Avagrado's Number: 6.02 x 10 23
The five types of chemical reactions are decomposition, combustion, anionic,single replacement,double replacements