1.1 particle theory and bonding\n1. water has 2 hydrogen and 1 oxygen atom - draw one molecule of water with…

1.1 particle theory and bonding\n1. water has 2 hydrogen and 1 oxygen atom - draw one molecule of water with the symbols and charges on the appropriate atoms.\n2. describe covalent bonding and draw a diagram showing the electrons.\n3. describe hydrogen bonding.\n4. draw three molecules of water with hydrogen bonding (make sure to use the 3 dots).\n5. describe ionic bonding and what happens between na and cl when they bond. include why the symbol for cl is negative and na is positive.\nexplain how polar molecules dissolve sodium chloride.

1.1 particle theory and bonding\n1. water has 2 hydrogen and 1 oxygen atom - draw one molecule of water with the symbols and charges on the appropriate atoms.\n2. describe covalent bonding and draw a diagram showing the electrons.\n3. describe hydrogen bonding.\n4. draw three molecules of water with hydrogen bonding (make sure to use the 3 dots).\n5. describe ionic bonding and what happens between na and cl when they bond. include why the symbol for cl is negative and na is positive.\nexplain how polar molecules dissolve sodium chloride.

Answer

Explanation:

Step1: Draw water molecule

Water ($H_2O$) has an oxygen atom covalently - bonded to two hydrogen atoms. Oxygen has 6 valence electrons, and it shares 2 electrons (one with each hydrogen) in covalent bonds. The Lewis structure has oxygen in the center with two single bonds to hydrogen atoms and two lone - pairs of electrons on the oxygen.

Step2: Describe covalent bonding

Covalent bonding is the sharing of electron pairs between atoms. In water, oxygen and hydrogen share electrons to achieve a stable electron configuration. Oxygen needs 8 valence electrons and hydrogen needs 2. By sharing electrons, they both satisfy their valence requirements.

Step3: Describe hydrogen bonding

Hydrogen bonding occurs when a hydrogen atom bonded to a highly electronegative atom (such as oxygen, nitrogen, or fluorine) is attracted to an electronegative atom in another molecule. In water, the partially positive hydrogen of one water molecule is attracted to the partially negative oxygen of another water molecule.

Step4: Draw hydrogen - bonding in water

Draw three water molecules. Show the hydrogen of one water molecule with a dotted line (representing the hydrogen bond) to the oxygen of another water molecule. Make sure to include the 3 dots for the lone - pairs on oxygen.

Step5: Describe ionic bonding in NaCl

Sodium (Na) has 1 valence electron and chlorine (Cl) has 7. Sodium donates its valence electron to chlorine. Na becomes $Na^+$ (a positive ion) and Cl becomes $Cl^-$ (a negative ion). The electrostatic attraction between these oppositely charged ions forms an ionic bond. When NaCl dissolves in water, the polar water molecules surround the ions. The partially negative oxygen of water is attracted to $Na^+$ and the partially positive hydrogen of water is attracted to $Cl^-$.

Step6: Explain dissolving of NaCl in water

The polar water molecules interact with the ions in sodium chloride. The oxygen end of water (negatively - charged) is attracted to the $Na^+$ ions and the hydrogen end (positively - charged) is attracted to the $Cl^-$ ions. This interaction overcomes the ionic bonds in NaCl, causing it to dissolve.

Answer:

  1. Lewis structure of water: O in the center with two single bonds to H and two lone - pairs on O.
  2. Covalent bonding is electron - sharing between atoms in water to achieve stable electron configurations.
  3. Hydrogen bonding is the attraction between H of one water molecule and O of another due to electronegativity differences.
  4. Draw three water molecules with dotted lines (hydrogen bonds) between H of one and O of another, with lone - pairs on O.
  5. Na donates an electron to Cl, forming $Na^+$ and $Cl^-$ which are attracted by electrostatic forces. In water, polar water molecules surround the ions for dissolution.
  6. Polar water molecules interact with $Na^+$ and $Cl^-$ ions, overcoming ionic bonds in NaCl for dissolution.