What is the electron configuration of neutral phosphorous What is the electron configuration of neutral phosphorous? 1s22s22p63s23p3 1s22s22p63s23p3 Phosphorous is located here

Atomic Trends How does atomic radius change down a group in the periodic table? It tends to increase.

Why is the radius of a positive ION always less than the radius of its NEUTRAL atom? It gave away an electron, and the nucleus pulls the remaining electrons in closer. Na neutral sodium 11 electrons 11 protons Na 1+ sodium ion 10 electrons 11 protons

What term is used to describe an atom's tendency to attract electrons (selfish of electrons) to itself when it is chemically combined with another element? electronegativity Really greedy because they are so close to having 8 valence electrons.

The noble gases don’t want or do much Which group of the periodic table has the highest electronegativity? 7A, the halogens The noble gases don’t want or do much More greedy for electrons More greedy for electrons

Which of the following elements has the lowest electronegativity (selfishness of electrons)? Choose the cation with the least valence electrons and the most amount of total electrons. More greedy for electrons More greedy for electrons

Electronegativity generally increases from left to right across a period. More greedy for electrons

Compared with the electronegativities of the elements at the left end of a particular period, the electronegativities of the elements at the right side of that same period (ROW) tend to be higher.

Which of the following factors contributes to the relatively greater atomic size of the higher-atomic-number elements within a particular family of the periodic table? More shielding of the outer electrons by the inner electrons

Groups (family or column) H As we go down a group each atom has another energy level More shielding The outer electrons have greater freedom from the nucleus. Li Na K Rb

Which of the following increases with increasing atomic number (GOING DOWN) in Group 2A? atomic radius…the electrons have more freedom to move outward because of shielding.

How does the shielding phenomenon affect the relative atomic sizes of elements in the same period (row)? Shielding has no effect on relative atomic size within a period. Na Mg Al Si P S Cl Ar

The one that is furthest right. Which of the following elements has the smallest atomic radius?

Atomic size generally decreases as you move from left to right across a period (row).

The energy required to remove an electron from a gaseous atom is called the ionization energy. Na neutral sodium 11 electrons 11 protons Na 1+ sodium ion 10 electrons 11 protons

When is an electron configuration particularly stable? When its last principle energy level is a filled.

For Group 3A metals, which electron is the most difficult to remove from a neutral atom? the fourth because it was meant to give away the three in the valence shell, but the fourth is going into an inner shell that was already stable.

Which of the following factors contributes to the huge ionization energy of the elements on the right side of a period in the periodic table? greater number of protons in nuclei and the number of valence electrons is so close to the number 8 Don’t want to give away electrons Don’t want to give away electrons

Which of the following elements has the smallest FIRST ionization energy? The elements in the 1A column because they are so anxious to get rid of that one valence electron. Don’t want to give away electrons Don’t want to give away electrons

As you move from left to right across the second period (row) of the periodic table the ionization energy increases Ionization energy increases because they don’t want to give away electrons Don’t want to give away electrons

Ionization energy needed & Electronegativity SIZE of atomic radius/diameter SIZE of atomic radius/diameter

pick positive cations before negative anions. Of the following atoms, which one has the smallest FIRST ionization energy? pick positive cations before negative anions. +1 +1 +3 +2 +1 +3 +2 +1 +2 +1 +2

Which of the following elements, would ionically bind to sulfur? metals bond with non-metals for an ionic bond. +1 +1 +3 +2 Back to REVIEW In document form +1 +3 S +2 +1 +2 +1 +2