1.3 Bonding and the Periodic Table Flashcards
Q: What is the arrangement of electrons in an atom called?
A: The arrangement of electrons is called the electron configuration, where electrons are distributed in “shells” or energy levels around the nucleus.
Q: Why are noble gas electronic structures significant?
A: Noble gases have full outer shells, making them stable and unreactive. Other elements often gain, lose, or share electrons to achieve the same stable configuration.
Q: What does the outermost electron shell determine?
A: The outermost shell, or valence shell, determines an element’s reactivity and chemical properties.
Q: How is the Periodic Table arranged?
A: The Periodic Table is arranged by increasing atomic number in rows (periods) and columns (groups) based on recurring chemical properties.
Q: What do elements in the same group of the Periodic Table have in common?
A: Elements in the same group have the same number of outer shell electrons, which gives them similar chemical properties.
Q: How does metallic character change across a period?
A: Metallic character decreases across a period from left to right as atoms hold onto their electrons more tightly.
Q: What are the properties of metals?
A: Metals are good conductors of heat and electricity, malleable, ductile, and tend to lose electrons to form positive ions.
Q: What are properties of non-metals?
A: Non-metals are** poor conductors**, brittle, and tend to gain or share electrons to form covalent bonds.
Q: How do group numbers relate to the number of valence electrons?
A: The group number for main group elements corresponds to the **number of valence electrons **(e.g., Group 1 has 1 valence electron).
Q: Why do elements in Group 1 and Group 17 react easily?
A: Group 1 elements lose 1 electron to achieve a stable configuration, while Group 17 elements gain 1 electron. Their reactivity is due to their desire to achieve a noble gas configuration.
