P.Table + Bonding

• What are the columns in the periodic table called?

  Groups
• What do elements in the same group have in common?

  Similar chemical properties
• What are the rows in the periodic table called?

  Periods
• How do properties change across a period?

  They change progressively
• Where are metals located in the periodic table?

  Left and center
• How do metals and non-metals differ in electron behavior?

  Metals lose electrons; non-metals gain or share
• What is the reactivity trend in Group 1 (Alkali Metals)?

  Reactivity increases down the group
• What is the reactivity trend in Group 7 (Halogens)?

  Reactivity decreases down the group
• What type of molecules do Group 7 elements form?

  Diatomic molecules
• Why are Group 0 (Noble Gases) unreactive?

  Due to full outer electron shells
• What do electrons do around the nucleus?

  Orbit in energy levels (shells)
• What determines the chemical properties of an element?

  Electron configuration
• How many electrons can the first shell hold?

  Up to 2 electrons
• How many electrons can subsequent shells hold?

  Up to 8 electrons
• What determines the group number of an element?

  Outer shell electrons
• What is the atomic number of Sodium (Na)?

  11
• What is the electron configuration of Sodium (Na)?

  2, 8, 1
• What group does Sodium belong to?

  Group 1
• What type of bonding occurs between metals and non-metals?

  Ionic bonding
• What happens to electrons during ionic bonding?

  They are transferred from metal to non-metal
• What is formed when a metal loses electrons?

  A positive ion (cation)
• What is formed when a non-metal gains electrons?

  A negative ion (anion)
• What type of bond is formed due to opposite charges attracting?

  A strong ionic bond
• What is the example of ionic bonding given in the material?

  Sodium chloride (NaCl)
• What type of bonding occurs between non-metals?

  Covalent bonding
• How do atoms achieve full outer shells in covalent bonding?

  By sharing electrons
• What is the example of covalent bonding given in the material?

  Water (H2O)
• How many hydrogen atoms share electrons with oxygen in water?

  Two hydrogen atoms
• What is the result of covalent bonding in water?

  A stable molecule with strong covalent bonds
• What are the types of covalent substances?

  1. Simple Molecular Substances:

  • Small molecules (e.g., H, CO, H2O)
  • Low melting and boiling points
  • Do not conduct electricity

  1. Giant Covalent Structures:

  • Large networks of atoms (e.g., diamond, graphite)
  • High melting and boiling points
  • Graphite conducts electricity; diamond does not
• Why do metals conduct electricity?

  Due to delocalized electrons in a lattice
• What property of metals allows for high malleability and ductility?

  Non-directional metallic bonds
• When do ionic compounds conduct electricity?

  When molten or dissolved
• Why do ionic compounds not conduct electricity when solid?

  Because ions are fixed in place
• What is the main characteristic of ionic compounds when molten?

  They conduct electricity