Unit 1 Chem Test

Ion- A negatively or positively charge atom

isotope- Atoms of the same element with different number of neutrons and mass numbers.

Where are the alkali metals on the periodic table?- 1st group

Where are the alkali earth metals on the periodic table?- 2nd group

What makes up the entire F block?- Metals

What is in the first row of the F block?- lanthanides

What’s in the second row of the F block- actinides

Where are the halogens on the periodic table- 7th group

Where are the noble gases- 8th group

Where are the transition metals on the periodic table?- d block

Ionization Energy- The amount o energy reached to remove the outermost electron from a species (atom or ion) in a gaseous state.

Electron Affinity- The energy released when an electron is added in the gas state.

Electronegativity- The ability of an atom to attract electrons when it is a compound

In a chemical compound the atom with the greater electronegativity… - more strongly attracts the bond’s electrons

Isotope-Atoms of the same element with different neutrons

Isoelectronic- having the same number of electrons or valence electrons

Orbital- when an electron is likely to be found in an atom

Excited State- The valence electron has moved from its ground state orbital to a higher energy orbital

Ground State- state in which the electrons in a atom, ion, or molecule are in the lowest energy levels possible

Effective Nuclear Charge- Atomic Radius

Aufbau Principle- electrons occupy lowest orbitals first

Pauli Exclusion Principle- only two electrons can occupy an orbital at the same time

Pauli Exclusion Principle #2- To occupy the same orbital, two electrons must have opposite spins

Pauli Exclusion Principle #3- An orbital holds two electrons that spin in opposite directions

Hund Rule- When electron fills orbitals of the same energy level, they do so in a way that maximize the particles with the same spin

Hund Rule #2- Single electrons occupy available orbitals first before doubling up