Refer to a periodic table. Which pair of elements do you expect to be most similar in their chemical properties? (LO 2.3) (a) K and Cu (b) O and Se (c) Be and B (d) Rb and Sr

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Step 1: Understand the concept of chemical properties similarity. Elements in the same group (column) of the periodic table have similar chemical properties because they have the same number of valence electrons.

Step 2: Identify the group for each element in the options.

Step 3: For option (a), K (Potassium) is in Group 1, and Cu (Copper) is in Group 11.

Step 4: For option (b), O (Oxygen) is in Group 16, and Se (Selenium) is also in Group 16.

Step 5: For option (c), Be (Beryllium) is in Group 2, and B (Boron) is in Group 13. For option (d), Rb (Rubidium) is in Group 1, and Sr (Strontium) is in Group 2.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Periodic Trends

Periodic trends refer to the predictable patterns in the properties of elements as you move across or down the periodic table. These trends include atomic radius, ionization energy, and electronegativity, which influence how elements interact chemically. Understanding these trends helps in predicting the behavior of elements and their similarities.

Group and Period Similarities

Elements in the same group (column) of the periodic table share similar chemical properties due to having the same number of valence electrons. This similarity affects their reactivity and the types of bonds they form. In contrast, elements in the same period (row) may have different properties as they have different valence electron configurations.

Metallic vs. Nonmetallic Properties

The distinction between metals and nonmetals is crucial for understanding chemical properties. Metals, typically found on the left side of the periodic table, are good conductors of heat and electricity and tend to lose electrons during reactions. Nonmetals, located on the right, are more likely to gain electrons. Recognizing these differences aids in predicting how elements will behave in chemical reactions.

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