2-chemistry of life
12. what is the difference between an element and a compound?
13. water is considered a polar molecule. what does that mean and what special properties does water possess because of its polarity?
14. in a cup of tea, what is the solvent? what is the solute?
15. what are the 3 subatomic particles that make up an atom? for each subatomic particle, include the mass and charge.

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Accepted Answer

### Question 12
# Brief Explanations:
An element is a pure substance made of only one type of atom (e.g., O, H). A compound is a pure substance made of two or more different elements chemically bonded (e.g., $H_2O$, $CO_2$). Elements can't be broken down chemically, compounds can (into elements).
# Answer:
An element is a pure substance composed of only one type of atom (e.g., oxygen, hydrogen). A compound is a pure substance composed of two or more different elements chemically bonded together (e.g., water $H_2O$, carbon dioxide $CO_2$). Elements cannot be broken down into simpler substances by chemical means, while compounds can be broken down into their constituent elements through chemical reactions.

### Question 13
# Brief Explanations:
A polar molecule has a partial positive and partial negative end (dipole) due to unequal electron sharing (e.g., $H_2O$: O is more electronegative, so O has $\delta^-$, H has $\delta^+$). Water’s polarity gives it properties: 1. Cohesion (water molecules stick to each other, causes surface tension). 2. Adhesion (sticks to other polar/charged surfaces, causes capillary action). 3. Universal solvent (dissolves polar/ionic substances, e.g., salts, sugars). 4. High specific heat (absorbs/retains heat, stabilizes temperature). 5. Less dense as solid (ice floats, insulates water bodies).
# Answer:
A polar molecule (like water) has a partial positive charge on one end and a partial negative charge on the other end due to unequal sharing of electrons between atoms (in $H_2O$, oxygen is more electronegative than hydrogen, so oxygen has a partial negative charge ($\delta^-$) and hydrogen has a partial positive charge ($\delta^+$).

Properties of water due to polarity:
1. **Cohesion**: Water molecules stick to each other (causes surface tension, e.g., insects walking on water).
2. **Adhesion**: Water molecules stick to other polar/charged surfaces (causes capillary action, e.g., water moving up plant stems).
3. **Universal Solvent**: Water dissolves polar/ionic substances (e.g., salts, sugars) because the $\delta^-$ and $\delta^+$ ends of water interact with charged ions or polar molecules.
4. **High Specific Heat**: Water absorbs/retains large amounts of heat (stabilizes temperatures in organisms and environments).
5. **Less Dense as a Solid**: Ice (solid water) is less dense than liquid water (due to hydrogen bonding structure), so it floats (insulates water bodies, protecting aquatic life).

### Question 14
# Brief Explanations:
In a solution, the solvent is the substance that dissolves others (usually the most abundant, liquid). The solute is the substance dissolved (usually less abundant, solid/liquid/gas). In tea, water is the solvent (dissolves tea solids, flavorings, etc.). The solute is the tea solids (e.g., tannins, flavor compounds) or any added substances (like sugar, tea leaves’ dissolved components).
# Answer:
In a cup of tea, the **solvent** is water (it is the substance that dissolves the other components). The **solute** is the tea solids (e.g., dissolved compounds from tea leaves, like tannins, flavor molecules) and any additional substances (e.g., sugar, milk solids if added) that are dissolved in the water.

### Question 15
# Brief Explanations:
The three subatomic particles in an atom are protons, neutrons, and electrons. Protons: +1 charge, mass ≈ 1 atomic mass unit (amu), located in the nucleus. Neutrons: 0 charge, mass ≈ 1 amu, located in the nucleus. Electrons: -1 charge, mass ≈ 0 amu (≈ $9.11 \times 10^{-31}$ kg), located in electron clouds/orbitals around the nucleus.
# Answer:
The three subatomic particles that make up an atom are:

1. **Proton**:
   - Charge: $+1$ (positive charge).
   - Mass: Approximately $1$ atomic mass unit (amu) (or $1.67 \times 10^{-27}$ kg).
   - Location: In the nucleus of the atom.

2. **Neutron**:
   - Charge: $0$ (neutral, no charge).
   - Mass: Approximately $1$ amu (or $1.67 \times 10^{-27}$ kg).
   - Location: In the nucleus of the atom.

3. **Electron**:
   - Charge: $-1$ (negative charge).
   - Mass: Approximately $0$ amu (or $9.11 \times 10^{-31}$ kg, much smaller than protons/neutrons).
   - Location: In electron clouds (orbitals) surrounding the nucleus.

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Question 12

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Question 13