Chemistry B: Lesson: CHARGING UP: IONIZATION OF ATOMS
If the valence electrons were removed, what would be the ion charge of the element? Na = _____ -1 +1 -3 +3
+1
If the valence electrons were removed, what would be the ion charge of the element? Mg = _____ -1 +1 -2 +2
+2
Al =
+3
Na =
1
Select the number of valence electrons for hydrogen.
1
Complete the chemical change. Na → Na+ +
1e-
What is the electron configuration when the valence electrons are removed from each of the elements listed in the chart? 1s22s22p63s2 1s22s22p6 1s22s2 1s22s22p63s1
1s22s22p6
Mg =
2
Al =
3
Select the number of valence electrons for carbon.
4
Select the number of valence electrons for nitrogen
5
Select the number of valence electrons for fluorine.
7
ion
A charged atom or particle
Complete the chemical change. +e- --> Cl-
Cl
Using the ideas from this section and the periodic table, choose the more reactive metal. Cs or Na
Cs
How is the ionization energy, E, related to a group of elements? E decreases from left to right. E decreases from right to left. E decreases from top to bottom. E decreases from bottom to top.
E decreases from top to bottom
How is E related to a period of elements? E generally increases from right to left. E generally decreases from right to left. E is constant within any given Period.
E generally decreses from right to left
valence electrons
Electrons from one atom that enter into reactions with electrons from a second atom
Using the ideas from this section and the periodic table, choose the more reactive nonmetal. C or F
F
Using the ideas from this section and the periodic table, choose the more reactive nonmetal. F or Cl
F
The energy necessary to overcome the attractions of electrons to the nucleus of an atom so as to remove electrons from the atom is called charging energy. True False
False
When all Group IIA elements lose their valence electrons, the remaining electron configurations are the same as for what family of elements? Family 1A, the Alkali Metals Family 2A, the Alkaline Metals Family 7A, the Halogens Family 8, the Noble Gases
Family 8, the Noble Gases
A charged atom or particle is called a(n) _______. muon ion isotope prion
Ion
Using the ideas from this section and the periodic table, choose the more reactive metal. K or Cu
K
Using the ideas from this section and the periodic table, choose the more reactive nonmetal. P or O
O
Why does the ionization energy change when moving down a group of elements? The number of valence electrons increases. The nuclear positive charge increases. The energy levels are increasing. The attractive force decreases as the atom gets larger.
The attractive force decreases as the atom gets larger.
What factor(s) may be responsible for the ionization energy within a period? Select all that apply. The valence electrons are further from the nucleus when moving from left to right. The valence electrons remain at the same distance from the nucleus when moving left to right. The diameter of the atom decreases somewhat as electrons are added. The attractive force of the nucleus increases.
The diameter of the atom decreases somewhat as electrons are added. The attractive force of the nucleus increases.
Ionization energy
The energy necessary to overcome the attractions of electrons to the nucleus of an atom so as to remove electrons from the atom in the gas phase
Which energy level requires the most energy to remove an electron? the shell containing valence electrons the next to outermost shell the innermost shell none of the above
The innermost shell
Ionization energy is required to remove an electron from an atom. True False
True
The two common units of E are electron volts and Kcal/mole. True False
True
Electrons located in the outermost shell of an atom are called
Valence
Using the ideas from this section and the periodic table, choose the more reactive metal. Al or Zn
Zn
The reactiveness of nonmetals depends on the atom's ability to
gain
Using the periodic table, find the neutral atom that has the same electron configuration as 1s22s22p6. boron neon phosphorus carbon
neon
How does the complete filling of a subshell affect E? no apparent effect produces chemical stability; therefore decreases E produces chemical stability; therefore increases E E becomes very high because the atom becomes inert
produces chemical stability; therefore increases E
What does the symbol "E3" represent? the energy of electrons in the third energy level the energy required to remove three of the outermost electrons the energy required to remove an electron in the third energy level the energy required to remove the third valence electron
the energy required to remove the third valence electron