which of the following statements are true
there are 2 polar covalent bonds in water
there are 3 ionic bonds in water
there is 1 ionic and 1 covalent bond in water
electrons are less attracted to oxygen than hydrogen
daaaaaaaaaaamn
The statement that is true is: "electrons are less attracted to oxygen than hydrogen."
To determine which of the statements are true, we need to understand the nature of chemical bonding in water.
Water (H2O) consists of two hydrogen atoms bonded covalently to one oxygen atom. Covalent bonds occur when atoms share electrons to fill their outermost energy levels.
Let's evaluate each statement:
1. "There are 2 polar covalent bonds in water": This statement is true. Water has two polar covalent bonds because the oxygen atom pulls the shared electrons closer to itself due to its higher electronegativity compared to hydrogen. This creates a partial negative charge on the oxygen atom and partial positive charges on the hydrogen atoms.
2. "There are 3 ionic bonds in water": This statement is false. Water does not contain ionic bonds. Ionic bonds occur between atoms with significantly different electronegativities, resulting in a transfer of electrons. In water, there is no transfer of electrons, so no ionic bonds are present.
3. "There is 1 ionic and 1 covalent bond in water": This statement is false. As mentioned earlier, water does not have any ionic bonds. It only has two polar covalent bonds between hydrogen and oxygen atoms.
4. "Electrons are less attracted to oxygen than hydrogen": This statement is false. In reality, electrons are more attracted to oxygen than hydrogen because of oxygen's higher electronegativity. Oxygen has a greater ability to attract electrons towards itself in a covalent bond, resulting in a partial negative charge on the oxygen atom and partial positive charges on the hydrogen atoms.
In conclusion, the only true statement is: "There are 2 polar covalent bonds in water."
Brenda -- it looks like you're trying to take short cuts in your online biology class. Read your text and try to find the answers yourself.
You're more likely to get help here if you post your answers along with the questions.