
Chem Periodic Table Trends final
Flashcard
•
Chemistry
•
8th - 11th Grade
•
Practice Problem
•
Hard
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15 questions
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1.
FLASHCARD QUESTION
Front
What are noble gases and why are they considered unreactive?
Back
Noble gases are elements in Group 18 of the periodic table that have filled valence electron shells, making them very stable and unreactive.
2.
FLASHCARD QUESTION
Front
Identify the period and group of arsenic in the periodic table.
Back
Arsenic is located in Period 4, Group 15 of the periodic table.
3.
FLASHCARD QUESTION
Front
What is the trend in ionization energy for group 1 metals and why does the 2nd ionization energy increase dramatically?
Back
The 2nd ionization energy for group 1 metals increases dramatically because removing a second electron results in a stable noble gas configuration.
4.
FLASHCARD QUESTION
Front
Describe the trend of atomic radius across a period in the periodic table.
Back
The atomic radius decreases from left to right within a period due to increasing nuclear charge, which pulls electrons closer to the nucleus.
5.
FLASHCARD QUESTION
Front
What does high electronegativity indicate about an atom's ability to attract electrons?
Back
Atoms with high electronegativity hold on to their electrons tightly, indicating a strong ability to attract electrons in a chemical bond.
6.
FLASHCARD QUESTION
Front
What is the significance of the periodic table's group number in relation to valence electrons?
Back
The group number of an element indicates the number of valence electrons it has, which influences its chemical properties and reactivity.
7.
FLASHCARD QUESTION
Front
Explain the concept of ionization energy and its periodic trend.
Back
Ionization energy is the energy required to remove an electron from an atom. It generally increases across a period and decreases down a group.
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