Periodic Trends Quiz
The modern periodic table shows the elements arranged in order of increasing atomic number.
v Arranged in this manner, the elements show a periodic pattern in their properties.
v This is why it’s called a Periodic table!
What this means is that certain groups of elements share similar physical & chemical properties.
v Periodically, as you run through the elements by increasing atomic number, you come across an element with similar properties to any element of your interest.
v This is similar to a calendar; as you run through the days by increasing number, you periodically come across a Monday, Wednesday, etc.
These periodic trends are due to the atoms’ composition and their desire to have a full outer energy level. Remember the octet rule: atoms desire to gain or lose e- to achieve 8 valence e- (to be like noble gases).
v Metals typically give up their e- (form positive ions) to be like the previous noble gas.
v Nonmetals typically gain more e- (form negative ions) to be like following noble gas.
Periodic Trends
1. Atomic Radius: Radius of atom without regard to surrounding atoms. (Size of the atom)
v Left to right, atomic radius ______________. The reason for this is _______________________
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v Top to bottom, atomic radius ______________. The reason for this is _____________________
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2. Ionic Radius: Radius of ion formed from atom. (Did it gain or lose electrons?)
v Left to right and top to bottom, ionic radius mostly follows the same trend as atomic radius (which should make sense – think about from where the ion comes).
v Positive ions are ______________ than the uncharged atom. The reason for this is ___________
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v Negative ions are ______________ than the uncharged atom. The reason for this is __________
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3. Electron Affinity: Attraction an atom has for an extra e-. (How much it wants to form a [-] ion.)
v Left to right, electron affinity ______________. The reason for this is ____________________
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v Top to bottom, electron affinity ______________. The reason for this is ___________________
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4. Ionization Energy: Energy needed to remove an e- from atom. (Energy needed to form a [+] ion.)
v Left to right, ionization energy ______________. The reason for this is ___________________
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v Top to bottom, electron affinity ______________. The reason for this is ___________________
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5. Electronegativity: Tendency of an element to pull e- toward itself in a bond. (Follows e- affinity trend)
v Left to right, electronegativity _______________. The reason for this is ___________________
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v Top to bottom, electronegativity _______________. The reason for this is _________________
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