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Chemistry Chapter 7
Terms in this set (14)
Why do the alkali metals react with the halogens in a 1:1 ratio? (Hint: Think about the
Alkali metals have a +1 charge and Halogens have a -1 charge. It would take one of each to achieve an overall net charge of 0 which is stable.
How did Dmitri Mendeleev arrange his periodic table?
In patterns of reactivity and properties that occur, "periodically."
What is effective nuclear charge?
The amount of attraction between the positively charged nucleus and the negatively charged out she'll electrons.
Why do noble gases tend to be unreactive?
They do not want to gain or lose electrons, therefore, no bonding takes place with these elements.
Why are Group 2 elements (such as calcium) less reactive than Group 1 elements (such as
More energy is required to lose two electrons than one electron.
Amount of energy needed to remove an electron from an atom.
General size of atom.
Amount of energy released or absorbed when an electron is added to an atom.
The ability of an atom to attract a shared electron to itself
Why are the trends for electronegativity and ionization energy similar?
They both are looking to reach the noble gases.
Explain the trend for ionization energy as you move down a group on the periodic table (from top to bottom). Why does this trend occur?
The energy becomes weaker and decreases as the group moves from the top to bottom.
Explain why sodium (Na) has a smaller radius than cesium (Cs).
Sodium has only three energy level rings compared to the six energy rings that Cesium has.
Explain why chlorine (Cl) has a higher electronegativity value than iodine (I).
Chlorine is smaller than Iodine.
Explain why rubidium (Rb) has a smaller ionization energy than fluorine (F).
Fluorine has the higher ionization level than Rubidium. Fluorine has larger atoms and the electrons are farther away. Effective nuclear charge of Rubidium is smaller than fluorines.
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