This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
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Activity 10.1: Classwork/Homework 1. Name the particle(s) found in the atom which: 1.1 Carry no electrical charge: Neutron 1.2 Has the smallest mass of all: Electron 1.3 Carry one positive electrical charge: Proton 1.4 Carry one negative electrical charge: Electron 1.5 Occur in the nucleus of the atom: Proton and Neutron 2. Define the following terms: 2.1 Nucleons: The particles found in the nucleus of an atom, which are protons and neutrons. 2.2 Mass number: The total number of protons and neutrons in the nucleus of an atom. 2.3 Atomic number: The number of protons in the nucleus of an atom, which determines the element's identity. 2.4 Relative atomic mass: The weighted average mass of the isotopes of an element, relative to (1)/(12) the mass of a carbon-12 atom. 3. Complete the table: | Element | Atomic number | Number of protons | Number of electrons | Number of neutrons | Mass number | | :------ | :------------ | :---------------- | :------------------ | :----------------- | :---------- | | ^12_6X (Carbon) | 6 | 6 | 6 | 6 | 12 | | ^16_8X (Oxygen) | 8 | 8 | 8 | 8 | 16 | | ^18_8X (Oxygen) | 8 | 8 | 8 | 10 | 18 | | ^31_16X (Sulfur) | 16 | 16 | 16 | 15 | 31 | | ^32_16X (Sulfur) | 16 | 16 | 16 | 16 | 32 | 4. Use the table completed in QUESTION 3 to answer the following questions. 4.1 The atomic number of an element is equal to the number of protons in a neutral atom of that element. 4.2 Similarity: Both the 4^th (^31_16X) and 5^th (^32_16X) elements have the same atomic number (16) and thus the same number of protons (16) and electrons (16). Difference: They have different mass numbers (31 vs 32) and different numbers of neutrons (15 vs 16). 4.3 We call atoms of elements with the same atomic number but different mass numbers isotopes. 4.4 First element (^12_6X): Carbon Second element (^16_8X): Oxygen Third element (^18_8X): Oxygen 5. Use the ^A_ZX notation to represent each of the following atoms: 5.1 Uranium-235: ^235_92U 5.2 Calcium-40: ^40_20Ca 6. A certain element Q has an atomic number of 10. It occurs as the following three isotopes: Q-20: 90,92%; Q-21: 0,26%; Q-22: 8,82% 6.1 An isotope is an atom of the same element (same number of protons) but with a different number of neutrons, resulting in a different mass number. 6.2 Element Q has an atomic number of 10, which corresponds to Neon. 6.3 The LEAST abundant isotope is Q-21 (0,26%). Step 1: Identify the mass number and atomic number. Mass number (A) = 21 Atomic number (Z) = 10 Step 2: Calculate the number of neutrons. Number of neutrons = Mass number - Atomic number Number of neutrons = 21 - 10 = 11 The number of neutrons in the nucleus of the least abundant isotope (Q-21) is 11. 6.4 Aufbau diagram for element Q (Neon, atomic number 10): Ne: 1s^2 2s^2 2p^6 The Aufbau diagram shows the electron configuration by filling orbitals in increasing order of energy. ` 1s: ↑↓ 2s: ↑↓ 2p: ↑↓ ↑↓ ↑↓ ` 6.5 The two rules applied when drawing the Aufbau diagram are: Aufbau Principle: Electrons fill atomic orbitals of the lowest available energy levels before occupying higher energy levels. Pauli Exclusion Principle: An atomic orbital can hold a maximum of two electrons, and these two electrons must have opposite spins. That's 2 down. 3 left today — send the next one.