Practice Atoms, Elements, and Compounds Exercise Question 1: Define the following terms: a) Atom b) Element c) Compound Answer 1: a) Atom: The smallest unit of an element that retains the properties of that element. It consists of a nucleus containing protons and neutrons, surrounded by electrons. b) Element: A pure substance made up of only one type of atom. It cannot be broken down into simpler substances by chemical means. c) Compound: A substance formed when two or more different elements chemically combine in fixed proportions. Compounds have different properties from their constituent elements. Question 2: Draw and label a simple diagram of an atom, including the nucleus, protons, neutrons, and electrons. Answer 2: This answer requires a diagram. Below is a textual representation. • Nucleus: Central part of the atom containing protons and neutrons. • Protons: Positively charged particles inside the nucleus. • Neutrons: Neutral particles inside the nucleus. • Electrons: Negatively charged particles orbiting the nucleus in shells. Question 3: Explain the difference between a molecule and a compound with examples. Answer 3: A molecule is a group of two or more atoms held together by covalent bonds. Molecules can consist of the same or different elements. For example, O2 (oxygen gas) is a molecule made of two oxygen atoms. A compound is a substance made of atoms of different elements chemically bonded together. For example, H2O (water) is a compound made of two hydrogen atoms and one oxygen atom. Question 4: Describe how the periodic table is organized, including the significance of groups and periods. Answer 4: The periodic table is organized into rows called periods and columns called groups. • Periods: Horizontal rows that indicate the number of electron shells in the atoms of the elements. • Groups: Vertical columns that contain elements with similar chemical properties due to having the same number of electrons in their outermost shell. Question 5: Write the chemical formula for the following compounds: a) Sodium chloride b) Carbon dioxide c) Magnesium oxide Answer 5: a) Sodium chloride: NaCl b) Carbon dioxide: CO2 c) Magnesium oxide: MgO Question 6: Balance the following chemical equation: H2+O2→H2O\text{H}_2 + \text{O}_2 \rightarrow \text{H}_2\text{O}H2+O2→H2O Answer 6: The balanced equation is: 2H2+O2→2H2O2\text{H}_2 + \text{O}_2 \rightarrow 2\text{H}_2\text{O}2H2+O2→2H2O Question 7: Differentiate between ionic and covalent bonds with examples. Practice Answer 7: • Ionic bonds: Formed when one atom transfers electrons to another atom, resulting in positively and negatively charged ions that attract each other. Example: NaCl (sodium chloride). • Covalent bonds: Formed when two atoms share electrons to achieve a full outer shell. Example: H2O (water). Question 8: Describe the structure of a water molecule and explain why it is considered a polar molecule. Answer 8: A water molecule consists of two hydrogen atoms covalently bonded to one oxygen atom. The oxygen atom has a higher electronegativity than hydrogen, causing the shared electrons to be more attracted to the oxygen. This creates a partial negative charge on the oxygen and a partial positive charge on the hydrogens, making water a polar molecule.