Question

name: ally m. chemistry semester 1 review sheet the purpose of this review sheet is to help prepare you for the final. it is important that you complete this with the intention of understanding the topics and not just having the correct answers. the questions on this review sheet are not the same as those on the exams; however, they are the same topics so understanding these questions will result in a much higher grade than those who do not understand these questions. there will be a couple of questions with graphs so you should also know how to read and interpret graphs. atomic structure: 1. what is the charge of protons, electrons, and neutrons? 2. how many protons, neutrons, and electrons are in a neutral tin - 119 atom? 3. what is the structure of an atom? what particles are in the nucleus? 4. what is the electron configuration of silver? 5. what happens to the electrons to produce colors during fireworks? 6. is energy absorbed or released when electrons move up energy levels to an excited state? 7. how do you calculate the average atomic mass of an element? 8. what is an isotope? 9. what particle determines the identity of an atom?

Explanation:

The problem is about chemistry concepts related to atomic structure. The subfield under Natural Science is Chemistry. Let's answer each question:

1. Charge of protons, electrons, neutrons: Protons have a positive charge ($+1$), electrons have a negative charge ($-1$), neutrons have no charge (neutral).
2. Tin - 119 atom: Tin (Sn) has an atomic number of 50. In a neutral atom, protons = electrons = 50. Neutrons = mass number - atomic number = 119 - 50 = 69.
3. Atomic structure and nucleus particles: An atom has a nucleus (containing protons and neutrons) and electrons in electron clouds/orbitals around the nucleus. Particles in the nucleus: protons and neutrons.
4. Electron configuration of Silver (Ag): Atomic number 47. Electron configuration: $1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^6 5s^1 4d^{10}$ (or the condensed form $[Kr] 5s^1 4d^{10}$).
5. Electrons in fireworks: Electrons in atoms of elements (in fireworks) absorb energy (from heat of explosion) and move to higher energy levels (excited state). Then, they release energy (as photons of light) when returning to lower energy levels, producing colors.
6. Energy for electrons moving up levels: Energy is absorbed. Moving to a higher energy level (excited state) requires energy input.
7. Calculating average atomic mass: Average atomic mass = $\sum$ (isotope mass $\times$ relative abundance (in decimal form)). For example, if an element has isotopes with masses $m_1, m_2, \dots$ and abundances $a_1, a_2, \dots$ (in decimal), then average mass = $m_1a_1 + m_2a_2 + \dots$.
8. Isotope definition: Isotopes are atoms of the same element (same atomic number, same number of protons) that have different mass numbers (different number of neutrons).
9. Particle determining atom identity: The number of protons (atomic number) determines the identity of an atom. Atoms with the same number of protons are the same element.

Answer:

1. Protons: +1 charge; Electrons: -1 charge; Neutrons: 0 charge.
2. Protons: 50, Neutrons: 69, Electrons: 50.
3. Atomic structure: Nucleus (protons + neutrons) and electrons in orbitals. Nucleus particles: protons, neutrons.
4. Electron configuration of Ag: $[Kr] 5s^1 4d^{10}$ (or full: $1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^6 5s^1 4d^{10}$).
5. Electrons absorb energy to excite, then release energy as light (photons) when de - exciting, producing colors.
6. Energy is absorbed.
7. Average atomic mass = sum of (isotope mass × relative abundance (decimal)).
8. Atoms of same element (same protons) with different neutrons (different mass numbers).
9. Number of protons (atomic number).