Ionic Bonds, simple molecules, covalent structures, metals

• At what temperature does table salt melt?

  801°C
• What charge does sodium ion have after losing an electron?

  Positive sodium ion (Na+)
• What charge does chloride ion have after gaining an electron?

  Negative chloride ion (Cl-)
• How do the opposite charges of sodium and chloride ions affect their bonding?

  Opposite charges keep them bonded as salt
• What type of structure do ionic compounds have?

  Lattice structure
• What are the main components of the crystal lattice structure shown?

  • Chloride ions (Cl-)
  • Sodium ions (Na+)
  • Ionic bonds between the ions
• Why can ionic compounds conduct electricity when molten or dissolved?

  The ions become free to move and carry current
• How many electrons are in the outer shell of a silicon (Si) atom?

  4
• What are the key characteristics of metals?

  • Made of metal atoms
  • Lose electrons to form positive ions
  • Form a lattice structure
  • Surrounded by delocalized electrons
  • Conduct heat and electricity easily
• What is the chemical formula for hydrogen sulfide?

  H2S
• What is the structure of silica in a giant covalent network?

  • Continuous structure
  • Atoms linked by strong covalent bonds
  • Silicon forms four bonds with oxygen
  • Repeating 3D pattern
• What are the four types of chemical bonding described in the image?

  • Ionic
  • Simple covalent
  • Network covalent
  • Metallic
• What structure do positive ions in metals form?

  Lattice structure
• How do giant covalent structures differ from simple molecules?

  They extend in every direction without breaks
• How do the electrical resistivity properties of the four bonding types differ?

  • Ionic: Very high electrical resistivity
  • Simple covalent: High electrical resistivity
  • Network covalent: Very high electrical resistivity
  • Metallic: Very low electrical resistivity
• What are the four main elements that make up the silicon dioxide molecule?

  Silicon, oxygen, covalent bonds, and outer shell of electrons
• What is the chemical formula for silicon dioxide (SiO2)?

  • Silicon (Si) atom forms 4 covalent bonds with 4 oxygen (O) atoms
  • The chemical formula is SiO2
• What is a simple molecule?

  A molecule formed by shared electrons
• What are the three main types of metal lattice structures?

  • Body-centered cubic (bcc)
  • Face-centered cubic (fcc)
  • Hexagonal
• How do the solubility properties of the four bonding types differ in water and organic solvents?

  • Ionic: High solubility in water, very low solubility in organic solvents
  • Simple covalent: Low solubility in water, very high solubility in organic solvents
  • Network covalent: Very low solubility in water and organic solvents
  • Metallic: Very low solubility in water and organic solvents
• What is the chemical formula for hydrogen bromide?

  HBr
• How do delocalized electrons contribute to metal properties?

  They maintain strong bond strength between atoms
• What is the chemical formula for nitrogen gas?

  N2
• Why do the ions in a compound form a crystal lattice structure?

  The ions are arranged in a lattice structure due to their ionic bonding
• How do atoms join to form a simple molecule?

  Through covalent bonds by sharing electrons
• How many covalent bonds are present in the silicon dioxide molecule?

  Four
• What is the hardness property of ionic bonding?

  high
• What is the hardness property of metallic bonding?

  low-high
• Why do giant covalent structures have very high melting points?

  They require much energy to break bonds
• What type of bonds are present in giant covalent structures?

  Covalent bonds
• What is the result of the regular arrangement of ions in ionic compounds?

  A strong, brittle crystal with a fixed shape
• How do simple molecules differ from ionic lattices?

  Simple molecules are discrete, ionic lattices are continuous
• How does the bonding in silicon dioxide contribute to its properties?

  Strong covalent bonds create a robust structure
• Why are metals strong despite being malleable?

  Metal ions can slide while maintaining bonding
• How are atoms arranged in a giant covalent network?

  Atoms are linked by strong covalent bonds in every direction
• What is the arrangement of atoms in a hexagonal structure?

  Stacked hexagonal layers
• Why can metals conduct heat and electricity easily?

  Due to shared delocalized electrons
• What causes ionic compounds to shatter when struck?

  Alignment of ions of the same charge
• How do giant covalent structures differ from ionic lattices in terms of weak points?

  They have no weak points like ionic lattices
• Why are simple molecules poor conductors of electricity?

  They lack free ions to carry charge