The electron in the metal atom goes from a higher energy level to a lower energy level.
The metal gives off black-body radiation.
The metal atom ionizes.
The electron in the metal atom goes from a lower energy level to a higher energy level.
Which one of these sets has the elements arranged in correct order of increasing atomic radius and correctly explains the basis for this order?
Hint: When electrons are being shielded (repelled) by one another, what does this do to the size of the atom?
Which one of these two elements is more likely to lose an electron than the other? Why?
[Ne]3s1 [Kr]5s2, 4d10, 5p5
Think: What is the trend in Ionizing Energy, Electron affinity and Atomic Radius? Atoms with stronger ionizing energy do WHAT to weak little punks like Lithium? A bigger Atomic Radius means it's easier to do what to an atom? Where is the Atomic Radius the largest?
Magnesium-Mg, Because it is easier to lose one electron and achieve Noble gas stability, than to gain 6.
Antimony-Sb, Because it has enough Ionizing Energy, it will drop the electron and achieve Noble gas stability.
Sodium-Na, Because it is easier to lose one electron and achieve Noble gas stability, than to gain 6.
Iodine-I, In losing an electron it will reach Noble gas stability.
The electron affinity for an atom A is greater than that of atom B. What can be inferred from the given statement?
Atom A gains electrons more easily than atom B.
Atom A has fewer valence electrons than atom B.
Atomic radius of atom A is larger than that of atom B.
Atom A loses electrons more easily than atom B.
Electron affinities of fluorine (F) and chlorine are –327.8 kJ/mol and –348.5 kJ/mol respectively. Which of the following statements can be inferred from the given statement?
Fluorine has fewer valence electrons than chlorine.
The atomic radius of fluorine is larger than that of chlorine.
Energy is absorbed when fluorine and chlorine atoms gain an electron.
Energy is released when fluorine and chlorine atoms gain an electron.
Which of the following statements is true?
Nonmetals gain electrons readily and hence have large electron affinity.
Nonmetals lose electrons readily and hence have low electron affinity.
Metals gain electrons readily and hence have low electron affinity.
Metals lose electrons readily and hence have large electron affinity.
The Transition Metals are the elements in Groups 1B and 3B through 8B. Transition Metals either have incompletely filled d subshells or readily lose electrons to achieve incompletely filled d subshells. According to this definition, which group of elements are not Transition Metals?
Hint: Attention to detail is key.
Group 9b - Zn, Cd, Hg
Group 2b - Cu, Ag, Au
Group 2b - Cu, Zn, Rg
Group 2b - Zn, Cd, Hg
True or False: The proccess of when an atom GAINS electrons to become an ion, is called Ionization
In drawing Lewis structures, a single line (single bond) between two elements represents?