🧪 Topic Summary
The periodic table organizes elements, including metals, based on their properties. Metal reactivity, or how easily a metal loses electrons to form positive ions, is directly related to its position on the periodic table. Generally, reactivity increases as you move down a group (vertical column) and towards the left across a period (horizontal row). This is because elements towards the bottom and left have a weaker hold on their outermost electrons.
Two key trends influence metal reactivity: Electronegativity (how strongly an atom attracts electrons) and Ionization Energy (the energy required to remove an electron). Metals with low electronegativity and low ionization energy are more reactive because they readily lose electrons to form positive ions.
🧱 Part A: Vocabulary
Match the term to its correct definition:
| Term |
Definition |
| 1. Electronegativity |
A. Energy required to remove an electron from an atom. |
| 2. Ionization Energy |
B. A positively charged ion. |
| 3. Reactivity |
C. The ability of a substance to undergo a chemical reaction. |
| 4. Cation |
D. How strongly an atom attracts electrons. |
| 5. Periodic Trend |
E. Predictable patterns of element properties based on position in the periodic table. |
✍️ Part B: Fill in the Blanks
Metals on the left side of the periodic table are generally more ______ than those on the right. As you move _______ a group, the reactivity of metals increases because the outermost electrons are further from the ______ and therefore easier to remove. Low _________ and low ionization energy contribute to higher metal reactivity.
🤔 Part C: Critical Thinking
Explain why potassium (K) is more reactive than sodium (Na), even though they are both in the same group on the periodic table. Be sure to include a discussion of atomic structure in your response.