In the following sets of elements, indicate which element has the smallest atomic size.

c. $\mathrm{N}, \mathrm{P}, \mathrm{As}$

How are the electron arrangements in a given group (vertical column) of the periodic table related? How is this relationship shown in the properties of the elements in the given group?

What is the Pauli exclusion principle?

When the electron in hydrogen is in the $n=$___ principal energy level, the atom is in its ground state.

What overall shape do the $2p$ and $3p$ orbitals have? How do the $2p$ orbitals differ from the $3p$ orbitals? How are they similar?

When an atom in an excited state returns to its ground state what happens to the excess energy of the atom?

Write the appropriate symbol for isotope $Z=11, A=23$

Write the atomic symbol ${ }_Z^A \mathrm{X}$ for the isotopes described as the isotope of boron with mass number 10

Write the atomic symbol $( ^{ A } _{ Z } X )$ for each of the isotopes described below. number of protons = 27, number of neutrons = 31.

The atomic particle that carries a positive charge is (a) the neutron. (b) the proton. ( c) the electron. (d) none of the above.

What contribution did these scientists make to atomic models of the atom?
(a) Dalton
(b) Thomson
(c) Rutherford

In the following sets of elements, which element would be expected to have the highest ionization energy?

a. $\mathrm{Cs}, \mathrm{K}, \mathrm{Li}$

What types of ions do the metals and the nonmetallic elements form? Do the metals lose or gain electrons in doing this? Do the nonmetallic elements gain or lose electrons in doing this?

The $\underline{~~~~~~~~~~}$ number represents the sum of the number of protons and neutrons in a nucleus.