test anything

• How is the periodic table arranged?

  In rows and columns based on atomic structure
• What are the horizontal rows in the periodic table called?

  Periods
• How many periods are in the periodic table?

  Seven periods
• What do the vertical columns in the periodic table represent?

  Groups or families of elements
• Why do elements in the same group behave similarly?

  They have the same number of outer electrons
• What is the reactivity of Group 1 elements?

  Very reactive, tend to lose one electron
• What are Group 17 elements known as?

  Halogens
• What does the number of periods correspond to in an atom?

  Number of energy levels or shells
• How many energy levels does Period 1 have?

  One energy level
• What happens to atomic radius across a period?

  It decreases from left to right
• Why does atomic radius decrease across a period?

  Increased nuclear charge pulls electrons closer
• Compare the atomic radius of lithium and fluorine.

  Lithium has a larger atomic radius than fluorine
• What is effective nuclear charge?

  The positive charge felt by outermost electrons
• Why does effective nuclear charge increase across a period?

  More protons with little added shielding
• What happens to atomic radius down a group?

  It increases as you move down
• Why does atomic radius increase down a group?

  Each element has an additional electron shell
• How many valence electrons do Group 1 elements have?

  One valence electron
• How do you determine valence electrons in Groups 13-18?

  Last digit of the group number
• What is the valence electron count for Group 17 elements?

  Seven valence electrons
• What is the reactivity trend for metals down a group?

  Reactivity increases down the group
• How does metal reactivity change across a period?

  Reactivity generally decreases from left to right
• Why are metals with fewer valence electrons more reactive?

  It's easier for them to lose outer electrons
• How does atomic radius affect metal reactivity?

  Larger atomic radius increases reactivity
• What is electronegativity?

  Tendency of an atom to attract electrons
• How do metals and nonmetals differ in electronegativity?

  Metals have low, nonmetals have high electronegativity
• What is ionization energy?

  Energy required to remove an electron
• What are the main periodic trends in the periodic table?

  • Atomic Radius
  • Ionization Energy
  • Electronegativity
  • Metallic Character
  • Reactivity
• What factors influence periodic trends?

  • Atomic Structure
  • Electron Arrangement
  • Nuclear Charge
  • Electron Shielding
• How do valence electrons relate to chemical reactivity?

  • Fewer valence electrons increase reactivity
  • Larger atomic radius increases reactivity
  • Similar valence configurations lead to similar properties
• How does reactivity change down the group in the periodic table?

  Reactivity increases from lithium to cesium
• What is the general trend of metal reactivity across a period?

  Reactivity decreases from left to right
• Which metals are more reactive, alkali and alkaline earth metals or transition metals?

  Alkali and alkaline earth metals
• Why do metals with fewer valence electrons tend to be more reactive?

  It's easier for them to lose outer electrons
• How does atomic radius affect metal reactivity?

  Larger atomic radius increases reactivity
• What is electronegativity?

  Tendency of an atom to attract electrons
• How does electronegativity change across a period?

  Electronegativity increases from left to right
• How does electronegativity change down a group?

  Electronegativity decreases from top to bottom
• How does electronegativity differ between metals and nonmetals?

  Metals have low, nonmetals have high electronegativity
• What is ionization energy?

  Energy required to remove an electron
• What is the first ionization energy?

  Energy to remove the first electron