1.8.2 Predicting element properties based on the periodic

• What is the atomic number of Argon (Ar)?

  18
• What is the atomic number of Neon (Ne)?

  10
• What is the atomic number of Oxygen (O)?

  8
• What is the atomic number of Beryllium (Be)?

  4
• What is the atomic number of Hydrogen (H)?

  1
• What do periods in the periodic table indicate?

  Energy levels of electrons
• What is the shape of the border between metals and non-metals?

  Staircase-shaped
• What does ductility in metals allow them to do?

  Be stretched into wires
• What is the appearance of metals described as?

  Shiny
• What happens to non-metals when they are hit?

  They break or shatter
• Which metal is excellent for electrical wiring?

  Copper
• What is the atomic number of Magnesium (Mg)?

  12
• How does the arrangement of elements in the periodic table help scientists?

  • Predict properties of elements
  • Understand chemical behavior
  • Identify trends in reactivity
• How do non-metals appear in terms of luster?

  They lack shiny luster
• What is the atomic number of Nitrogen (N)?

  7
• What is a hard non-metal that is brittle?

  Diamond
• Which period has the lowest energy level of electrons?

  Period 1
• What is the atomic number of Sodium (Na)?

  11
• How do groups help in predicting element properties?

  They show similar properties based on electron configuration
• What is the atomic number of Krypton (Kr)?

  36
• How are most metals characterized in terms of density?

  Heavy for their size
• How do the trends in atomic radius, ionization energy, and electron affinity relate to the classification of elements as metallic, nonmetallic, or metalloid?

  • Metallic character increases from right to left
  • Nonmetallic character increases from left to right
  • Metalloids lie between metals and nonmetals
• What state are metals usually in at room temperature?

  Solid
• What trend occurs in ionization energy down groups?

  Ionization energy decreases
• Which two non-metals are gases at room temperature?

  Oxygen and chlorine
• What are the trends in atomic radius, ionization energy, and electron affinity across the periodic table?

  • Atomic radius increases from top to bottom and left to right
  • Ionization energy decreases from top to bottom and increases from left to right
  • Electron affinity decreases from top to bottom and increases from left to right
• What trend occurs in electronegativity across periods?

  Electronegativity increases
• What are the two main structures of the periodic table?

  Periods and groups
• Why are metals valuable in various applications?

  • Due to their conductivity
  • Malleability allows for versatile shaping
  • Ductility enables wire production
  • Luster enhances aesthetic appeal
  • Density provides structural strength
• What is the atomic number of Fluorine (F)?

  9
• What types of elements are found on the right side of the periodic table?

  Non-metals, including gases and solids
• Why is the resolution limit of a light microscope 0.2 µm?

  Because it is the wavelength of visible light
• Where are metals primarily located in the periodic table?

  Mostly on the left side
• What are the two specific groups of metals mentioned?

  Transition metals and lanthanides
• How does the reactivity of metals and non-metals compare in the periodic table?

  Metals become more reactive from left to right, while non-metals become less reactive from right to left
• What is the relationship between atomic radius and electron affinity?

  As atomic radius increases, electron affinity decreases
• What is a characteristic of Group 1 elements?

  They have one electron in their outer shell
• What are the vertical columns in the periodic table called?

  Groups
• What types of elements are classified as metalloids?

  Elements along the staircase border
• Why are Group 1 elements considered reactive metals?

  Due to having one electron in their outer shell