Atomic Blueprint A targeted chemistry review and practice bundle covering atomic structure, isotopes, mass spectrometry, electron configurations, periodic families, matter classification, and physical versus chemical changes. Includes interactive review slides, a comprehensive concept review guide, an assessment-style practice worksheet, and a detailed teacher solutions guide.
T timothy.nixon
Atomic Blueprint Review Guide
A comprehensive two-page chemistry review guide synthesizing atomic structure, isotopic notation, mass spectrometry calculations, electron configurations, periodic table families, matter classification, and separation techniques. Designed with tight layout hierarchy and clean visual tables.
Atomic Blueprint Practice Worksheet
An authentic assessment-style chemistry practice worksheet featuring 18 rigorous questions patterned after the Q1 Interim Assessment. Covers periodic trends, subatomic accounting, particle-level models, mixture separation flowcharts, mass spectrometry calculations, and orbital diagrams.
Atomic Blueprint Review Slides
A six-slide interactive review deck for the chemistry interim assessment. Covers atomic structure, mass spectrometry weighted averages, orbital configurations, periodic families, and matter separation schemes with clear guided practice prompts.
Atomic Blueprint Solutions Guide
A comprehensive two-page teacher solutions and scoring guide for the Atomic Blueprint Practice Worksheet. Features complete worked answers, subatomic particle inventory keys, conceptual rationales, common student misconceptions, and an interim assessment alignment matrix.
Atomic Blueprint A targeted chemistry review and practice bundle covering atomic structure, isotopes, mass spectrometry, electron configurations, periodic families, matter classification, and physical versus chemical changes. Includes interactive review slides, a comprehensive concept review guide, an assessment-style practice worksheet, and a detailed teacher solutions guide.
T timothy.nixon
Atomic Blueprint Review Guide Unit 1 Review High School Chemistry
Atomic Blueprint Review Guide
Foundational Principles: Atomic Structure, Mass Spectrometry & Electron Configurations
Name: ______________________
Period: _____ Date: _________
1. Atomic Architecture & Subatomic Inventory
Proton (\(p^+\))
Charge: +1 | Mass: ~1 amu
Defines elemental identity (Atomic # \(Z\)). Fixed in chemical changes.
Neutron (\(n^0\))
Charge: 0 | Mass: ~1 amu
In nucleus with \(p^+\). Determines isotopes & mass number (\(A - Z\)).
Electron (\(e^-\))
Charge: -1 | Mass: ~0 amu
Fills >99.9% volume (empty space). Governs charge & bonding.
\(^{A}_{Z}\text{X}^{q}\)
\(A\) (Mass #): \(p^+ + n^0\) | \(Z\) (Atomic #): \(p^+\)
\(q\) (Charge): \(p^+ - e^-\) (\(0\) if neutral)
• Isotopes: Same \(Z\) (\(p^+\)), different \(n^0\) (diff. mass). Same chemical nature!
• Cation (+): Lost \(e^-\) (\(p^+ > e^-\)) | Anion (-): Gained \(e^-\) (\(e^- > p^+\))
2. Mass Spectrometry & Average Atomic Mass
Interpreting Mass Spectra
• X-axis (\(m/z\)): Mass-to-charge ratio \(\approx\) Isotopic mass in amu.
• Y-axis (% Abundance): Relative amount of each isotope.
• Peak count: Number of stable natural isotopes.
• Tallest peak: Dominant isotope; atomic mass lies closest to it.
• Single peak: Monoisotopic element (e.g. peak at 19 amu = \(^{19}\text{F}\)).
Weighted Average Formula
\(\text{Avg Mass} = \sum (\text{Fractional Abundance} \times \text{Isotopic Mass})\)
Correct numerical setup: Multiply decimal percent by mass, then add:
Boron (19.78% $^{10}\text{B}$ at 10.01 amu, 80.22% $^{11}\text{B}$ at 11.01 amu):
3. Electron Architecture & Periodic Blocks
Aufbau Principle
Electrons fill lowest available energy orbital first: \(1s \to 2s \to 2p \to 3s \to 3p \to 4s \to 3d\).
Hund’s Rule
Degenerate orbitals (\(p, d\)) fill singly with parallel spins before pairing up (\([\uparrow][\uparrow][\uparrow]\)).
Pauli Exclusion
Max 2 electrons per orbital, and they must have opposite spins (\(\uparrow\downarrow\)).
• Oxygen Ground State (\(8e^-\)): \(1s^2 2s^2 2p^4\) \(\to\) \(2p\) orbital box: \([\uparrow\downarrow][\uparrow\ ][\uparrow\ ]\)
• Valence Notation: \(ns^2 np^1 \to 3\) valence \(e^-\) = Group 13 (Boron column).
• Transition Metals: Highest energy electrons reside in \(d\)-subshell (e.g., \(4s^2 3d^3\)).
• Forbidden Subshells: “\(2d\)” does not exist (\(n=2\) only has \(s\) and \(p\)).
• Isoelectronic Ions: \(\text{K}^+\) (18 \(e^-\)) shares configuration with neutral \(\text{Ar}\).
• Halide / Alkaline Ions: Halogens gain 1 \(e^-\) (\(s^2 p^6\)); Group 2 lose 2 \(e^-\) (\(s^2 p^6\)).
Chemistry Q1 Interim Preparation Page 1 of 2 Matter, Atoms & Quantized Electrons
Unit 1 Review — Reference Part 2
Periodic Families, Matter Classification & Reactions
High School Chemistry
4. Periodic Families & Laboratory Properties
Family Group / Valence Chemical & Physical Behaviors Lab / Safety Notes Alkali Metals Group 1 (\(ns^1\)) Most reactive metals; soft; form \(+1\) cations; good conductors. React violently with \(H_2O\)! Store under mineral oil. Damp paper towel causes fire! Alkaline Earth Group 2 (\(ns^2\)) Reactive metals; form \(+2\) cations (\(\text{Mg}^{2+}, \text{Ca}^{2+}\)); basic oxides. React moderately with hot water/acid; less vigorous than Group 1. Transition Metals Groups 3–12 (\(d\)-block) Hard metals; high melting points; multiple oxidation states; colored compounds. Highest energy electrons occupy \((n-1)d\) subshells. Good conductors. Halogens Group 17 (\(ns^2 np^5\)) Most reactive nonmetals; form \(-1\) anions; all 3 states of matter at STP. \(F_2, Cl_2\) (gas); \(Br_2\) (liquid); \(I_2\) (solid). Corrosive oxidizers. Noble Gases Group 18 (\(ns^2 np^6\)) Completely unreactive/inert; full octet; monoatomic gases. Extremely high ionization energy; zero tendency to form bonds.
5. Matter Classification & Separation Schemes
Classification Framework
• Pure Substance: Uniform composition. Cannot be separated physically.
- Element: 1 type of atom (\(Na, O_2\)). Cannot be broken down chemically or physically.Compound: 2+ chemically bonded elements (\(NaHCO_3, H_2O\)). Broken down only by chemical reactions.
• Mixture: Physical blend of 2+ substances. Retain individual identities.
- Heterogeneous: Non-uniform distribution (solids, suspensions).Homogeneous: Uniform solution down to molecular scale (salt water, air).
Separation Techniques
<table class="w-full text-left text-[9.5px] text-slate-700"><tbody><tr class="border-b border-slate-100"><td class="font-bold py-0.5 text-slate-900">Magnetism:</td><td>Pulls magnetic solids (e.g., \(Nd, Fe\)) from non-magnetic matrix.</td></tr><tr class="border-b border-slate-100"><td class="font-bold py-0.5 text-slate-900">Filtration:</td><td>Separates insoluble solids from liquid phase via pore size.</td></tr><tr class="border-b border-slate-100"><td class="font-bold py-0.5 text-slate-900">Temp Solubility:</td><td>Solutes dissolving only at high temp (e.g. >45°C) isolate selectively upon cooling/heating.</td></tr><tr><td class="font-bold py-0.5 text-slate-900">Boiling / Evap:</td><td>Separates volatile solvent from non-volatile solute by boiling point (e.g., alcohol bp 78°C).</td></tr></tbody></table>
6. Physical vs. Chemical Changes (Particle Modeling)
Physical Change
• Core Rule: Chemical identity and intramolecular bonds remain intact.Sublimation (\(CO_2(s) \to CO_2(g)\)): Dry ice molecules do NOT break into separate C and O atoms! Molecular composition is 100% conserved; particles merely spread apart into random gas motion.Syringe Compression: Decreasing volume crowds molecules together without altering gas stoichiometry or identity.
Chemical Change
• Core Rule: Chemical bonds break and form; produces new substances with distinct identities and properties.Precipitation: \(AgNO_3(aq) + KCl(aq) \to AgCl(s) + KNO_3(aq)\). Solvated ions organize into an insoluble new crystalline solid.Key Evidence: Formation of precipitate, unforced color change, gas evolution, dramatic heat release.
Interim Assessment Exam Alerts
1. Isotope vs Ion: Isotopes have identical protons, different neutrons. Changing protons changes the element!
2. Sublimation Trap: Sublimation does NOT split \(CO_2\) into atoms. Look for intact triatomic clusters spaced out.
3. Mass Spec Reading: Peak height = abundance, NOT atomic number. The tallest peak is the most abundant isotope.
Chemistry Q1 Interim Preparation Page 2 of 2 Periodic Trends, Matter & Chemical Reactions
Atomic Blueprint Practice Worksheet Interim Prep High School Chemistry
Atomic Blueprint Practice Worksheet
Part I: Periodic Families, Subatomic Particles & Particle-Level Transformations
Name: ______________________
Date: _________ Period: _____
Set 1: Periodic Families & Laboratory Safety Questions 1–4
Use choices (A)–(D) for Questions 1–3. Each choice may be used once, more than once, or not at all:
(A) Alkali metals
(B) Alkaline earth metals
(C) Halogens
(D) Noble gases
Contains elements in solid, liquid, and gas states at STP:
Choice: [ _____ ]
Full valence octet and negligible chemical reactivity:
Choice: [ _____ ]
Soft metals that react violently with moisture to form \(+1\) ions:
Choice: [ _____ ]
4. A student attempts to test electrical conductivity by cutting sodium stored under mineral oil. Before testing, the student wipes the metal with a damp paper towel. Why is this action hazardous?
(A) Water dissolves sodium metal into non-conductive sand particles.
(B) Water reacts vigorously with sodium, producing caustic NaOH and flammable H₂ gas.
(C) Water cools the sodium below its superconductive threshold temperature.
(D) Water instantly oxidizes sodium into an inert noble gas compound.
Set 2: Subatomic Accounting & Nuclear Symbols Questions 5–7
5. Complete the subatomic table for each independent species below:
Species Notation Atomic # (\(Z\)) Mass # (\(A\)) Protons (\(p^+\)) Neutrons (\(n^0\)) Electrons (\(e^-\)) Net Charge \(^{238}_{\ 92}\text{U}\) 92 238 92 ______ ______ 0 \(^{80}_{35}\text{Br}^{-}\) 35 80 ______ 45 ______ -1 \(^{27}_{13}\text{Al}^{3+}\) 13 ______ 13 14 ______ +3
6. Which statement regarding atomic structure is FALSE?
(A) The nucleus holds essentially all the atomic mass.
(B) Electrons occupy virtually all of the atom's total volume.
Atomic Blueprint Review Slides Unit 1 Review High School Chemistry
Interim Assessment Prep
Atomic Blueprint:
Chemistry Mastery & Review
Key concepts, mathematical setups, and particle-level reasoning across atomic structure, mass spectrometry, and matter classification.
Subatomic Inventory
Mass Spec & Averages
Electron Configurations
Concept Anchor 1
Subatomic Inventory & Isotope Rules
\(^{A}_{Z}\text{X}^{q}\)
Core Subatomic Rules
• Protons (\(Z\)): Fixes elemental identity. Cannot change!
• Neutrons (\(n^0\)): \(\text{Mass Number }(A) - \text{Protons }(Z)\).
• Electrons (\(e^-\)): \(\text{Protons }(Z) - \text{Charge }(q)\).
• Isotopes: Same \(p^+\), different \(n^0\). Identical chemistry!
Guided Quick Check
Analyze \(^{243}_{\ 95}\text{Am}^{3+}\):
Protons = 95 (Atomic # \(Z\))
Neutrons = \(243 - 95 =\) 148
Electrons = \(95 - 3 =\) 92 (\(+3\) cation)
Remember: Positive charge means electrons were lost, not protons gained!
Key Exam Principle: Protons define the atom Slide 2 of 6
Concept Anchor 2
Mass Spectrometry & Average Mass
Weighted Average Setup
Reading the Spectrum
• X-axis (\(m/z\)): Gives the mass of each isotope in amu.
• Y-axis: Relative abundance (tallest peak = most common).
• Single Peak: Only 1 isotope exists (e.g. \(^{19}\text{F}\)).
Exam Calculation Setup
To calculate average atomic mass, convert percentages to decimals and sum products:
\(\text{Avg Mass} = (\%_1)(\text{mass}_1) + (\%_2)(\text{mass}_2)\)
Exam Trap: Never multiply percentages directly together or take a simple unweighted mean!
Tallest peak pulls the average closest to its mass value Slide 3 of 6
Concept Anchor 3
Electron Configurations & Quantum Rules
Aufbau • Hund • Pauli
Aufbau Principle
Fill lowest energy orbitals first:
Trap: "2d" does NOT exist!
Atomic Blueprint Solutions Guide Teacher Key & Solutions High School Chemistry
Atomic Blueprint Solutions Guide
Complete Rationales, Subatomic Calculations & Misconception Diagnostics
Master Scoring Guide
Unit 1 Interim Preparation
Set 1 Solutions: Periodic Families & Lab Safety Test Items Q1–4, Q23 Alignment
1. Answer: (C) Halogens
Rationale: At 25°C, \(F_2\) and \(Cl_2\) are gases, \(Br_2\) is a reddish-brown liquid, and \(I_2\) is a dark purple solid.
2. Answer: (D) Noble gases
Rationale: Completely filled valence shell (\(ns^2 np^6\)) confers thermodynamic stability; inert under normal conditions.
3. Answer: (A) Alkali metals
Rationale: Low first ionization energy drives loss of the single valence \(s\) electron to form stable \(+1\) cations.
4. Answer: (B) Water reacts vigorously with sodium to produce caustic NaOH and flammable H₂
Pedagogical Note: Students must recognize that alkali metals react exothermically with water: \(2\text{Na}(s) + 2\text{H}_2\text{O}(l) \to 2\text{NaOH}(aq) + \text{H}_2(g)\). Storing under oil excludes both moisture and oxygen. Using wet materials is a critical safety violation.
Set 2 Solutions: Subatomic Accounting & Nuclear Symbols Test Items Q5, Q9, Q10, Q17 Alignment
5. Completed Subatomic Inventory Key:
Species \(Z\) \(A\) \(p^+\) \(n^0\) (\(A-Z\)) \(e^-\) (\(p^+ - q\)) Charge (\(q\)) \(^{238}_{\ 92}\text{U}\) 92 238 92 146 92 0 \(^{80}_{35}\text{Br}^{-}\) 35 80 35 45 36 -1 \(^{27}_{13}\text{Al}^{3+}\) 13 27 13 14 10 +3
6. Answer: (C) Isotopes have different proton counts
Why False: If proton count changes, the atomic identity changes entirely. Isotopes have identical protons, differing only in neutrons.
7. Answer: (A) Isotopes of sulfur with different mass numbers
Rationale: Both have \(16p^+\) (Sulfur). Atom X has \(A = 16+16=32\); Atom Y has \(A = 16+18=34\). They are \(^{32}\text{S}\) and \(^{34}\text{S}\).
(C) Isotopes of an element have different proton counts.
(D) Neutral atoms always possess equal protons and electrons.
7. Atom X has (16p, 16n, 16e); Atom Y has (16p, 18n, 16e). They are:
(A) Isotopes of sulfur with different mass numbers.
(B) Two completely different chemical elements.
(C) Isoelectronic ions with different charges.
(D) Allotropes differing only in electron energy shells.
Set 3: Particle Diagrams & Transformations Questions 8–9
8. Dry ice (\(\text{CO}_2\)) sublimes into gas. Which statement best explains the particle-level change?
(A) Chemical change: \(\text{C}-\text{O}\) bonds break to form free carbon and oxygen atoms.
(B) Physical change: intermolecular spacing increases while \(\text{CO}_2\) molecules stay intact.
(C) Chemical change: \(\text{CO}_2\) molecules rearrange into a new compound with different properties.
(D) Physical change: \(\text{CO}_2\) splits into diatomic \(\text{C}_2\) and \(\text{O}_2\) molecules.
9. When \(\text{Pb(NO}_3)_2(aq)\) and \(2\text{KI}(aq)\) mix, a bright yellow \(\text{PbI}_2(s)\) solid precipitates:
(A) Physical change: the reactants are simply mixed and can be separated by filtration without altering bonds.
(B) Chemical change: new ionic bonds form to produce a new substance with unique chemical properties.
(C) Physical change: change of state from aqueous to solid indicates only phase transition.
(D) Chemical change: potassium atoms lose all their protons to iodine atoms.
Chemistry Interim Practice Worksheet Page 1 of 2 Periodic Table & Subatomic Dynamics
Separation Schemes, Mass Spectrometry & Electron Structure Set 4: Mixture Separation Scheme Questions 10–12
A solid mixture of Iron powder (\(\text{Fe}\)) , Potassium chloride (\(\text{KCl}\)) , and Silicon dioxide sand (\(\text{SiO}_2\)) is separated according to the flowchart below:
Substance 1
Substance 2
Substance 3
Substance 1 is isolated purely based on which property?
If \(\text{KCl}\) is soluble in water and sand is insoluble, Substance 2 is:
(A) \(\text{KCl}\) crystals
The initial 3-substance blend is a _____ mixture; the filtrate before evaporation is a _____ mixture.
(A) heterogeneous; homogeneous
(B) homogeneous; heterogeneous
(C) homogeneous; homogeneous
(D) heterogeneous; heterogeneous
Set 5: Mass Spectrometry Analysis Questions 13–15
Mass Spectrum of Unknown Element Q 0 50 100% 84 86 87 88 82.6%
Which numerical setup correctly calculates the average atomic mass?
(A) \((0.0056)(84) + (0.0986)(86) + (0.0700)(87) + (0.8258)(88)\)
(B) \((84 + 86 + 87 + 88) \div 4\)
(C) \([(84)(0.56)] \times [(86)(9.86)] \times [(87)(7.00)] \times [(88)(82.58)]\)
With calculated mass \(\approx 87.62\text{ amu}\), Element Q is most likely:
(A) \(\text{Rb}\) (85.47)
(B) \(\text{Sr}\) (87.62)
(D) \(\text{Zr}\) (91.22)
Set 6: Electron Configurations & Quantum Principles Questions 15–18
Which electron configuration is impossible ?
(A) \(1s^2 2s^2 2p^6 3s^1\)
(B) \(1s^2 2s^2 2p^6 2d^4 3s^2\)
(C) \(1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^5\)
(D) \(1s^2 2s^2 2p^6 3s^2 3p^6\)
Which particle is isoelectronic with \(\text{S}^{2-}\)?
(A) Oxygen atom (\(\text{O}\))
(B) Neon atom (\(\text{Ne}\))
(C) Argon atom (\(\text{Ar}\))
(D) Magnesium ion (\(\text{Mg}^{2+}\))
Ground state valence configuration \(ns^2 np^3\) is in:
Ground state nitrogen (\(1s^2 2s^2 2p^3\)) orbital diagram:
(A) 2s: \([\uparrow\downarrow]\) 2p: \([\uparrow\downarrow][\uparrow\ ][\ \ ]\)
(B) 2s: \([\uparrow\downarrow]\) 2p: \([\uparrow\ ][\uparrow\ ][\uparrow\ ]\) (parallel)
(C) 2s: \([\uparrow\downarrow]\) 2p: \([\uparrow\ ][\downarrow][\uparrow\ ]\)
(D) 2s: \([\uparrow\ ]\) 2p: \([\uparrow\downarrow][\uparrow\downarrow][\ \ ]\)
Chemistry Interim Practice Worksheet Page 2 of 2 Mass Spectrometry, Flowcharts & Orbitals
Hund's Rule Orbitals of same energy fill singly with parallel spins before pairing up.
Oxygen \(2p^4\): \([\uparrow\downarrow][\uparrow\ ][\uparrow\ ]\)
Periodic Blocks • \(ns^2 np^1 \to\) Group 13
\(\text{K}^+\) is isoelectronic with \(\text{Ar}\)
Isoelectronic species share the same total electron count Slide 4 of 6
Matter Classification & Separation Logic
Phase & Chemical Changes
• Sublimation (\(\text{CO}_2(s) \to \text{CO}_2(g)\)): Purely physical! Triatomic molecules stay intact.
• Precipitation (\(\text{Ag}^+ + \text{Cl}^- \to \text{AgCl}(s)\)): Chemical! New bonds, new substance.
• Pure Element: Cannot be decomposed chemically or physically.
Flowchart Separation Strategy Step 1: Magnetism removes ferromagnetic solids.
Step 2: Water + Filtration separates soluble from insoluble.
Step 3: Boiling point differences allow distillation.
Physical separation techniques exploit differences in physical properties Slide 5 of 6
Mastery Checklist & Independent Practice
Review Guide Keep your 2-page reference sheet out to check formulas, families, and key rules.
Worksheet Check Complete the 18 authentic assessment-style problems on the practice worksheet.
Error Analysis Review step-by-step solutions and eliminate common multiple-choice traps.
Goal: 100% Accuracy on Atomic & Matter Concepts Slide 6 of 6
Set 3 Solutions: Particle Transformations Test Items Q6, Q7–8, Q11 Alignment
8. Answer: (B) Physical change; \(\text{CO}_2\) molecules stay intact
Key Concept: Sublimation (\(s \to g\)) disrupts weak intermolecular forces, not covalent \(\text{C}=\text{O}\) bonds. The molecular identity remains \(\text{CO}_2\).
9. Answer: (B) Chemical change; new ionic bonds form
Key Concept: Aqueous \(\text{Pb}^{2+}\) and \(\text{I}^-\) ions form insoluble \(\text{PbI}_2(s)\) crystal lattice with distinct properties from the original soluble salts.
Chemistry Interim Solutions Guide Page 1 of 2 Subatomic Accounting & Particle Models
Teacher Key & Solutions — Part II
Mixtures, Mass Spectrometry & Quantum Architecture Scoring & Alignment Matrix
Set 4 Solutions: Mixture Separation Flowchart Test Items Q13–16 Alignment
10. Answer: (B) Ferromagnetism
Iron powder is pulled out by the magnetic field; all other components are diamagnetic/non-magnetic.
11. Answer: (C) Sand (\(\text{SiO}_2\))
Sand is completely insoluble in water and is trapped as residue on the filter paper while \(\text{KCl}\) dissolves.
12. Answer: (A) Heterogeneous; homogeneous
Initial blend has visible distinct phases (heterogeneous); the filtered \(\text{KCl}(aq)\) is uniform down to the ion level (homogeneous).
Set 5 Solutions: Mass Spectrometry Analysis Test Items Q18, Q22, Q29–31 Alignment
13. Answer: (A) Correct Weighted Setup
\((0.0056)(84) + (0.0986)(86) + (0.0700)(87) + (0.8258)(88)\)
Abundances must be converted to fractional decimals (\(\% \div 100\)) and multiplied by respective isotopic masses before summing.
14. Answer: (B) Strontium (\(\text{Sr}\), 87.62 amu)
Reasoning: Peak 88 dominates (82.6%), pulling the weighted average close to 88 (specifically 87.62 amu), matching Strontium in Group 2.
Set 6 Solutions: Electron Configurations & Orbitals Test Items Q20, Q21, Q24–28 Alignment
15. Answer: (B) \(1s^2 2s^2 2p^6 2d^4 3s^2\) is impossible
Quantum Rule: The \(n=2\) principal energy level only has \(\ell=0\) (\(s\)) and \(\ell=1\) (\(p\)) orbitals. \(d\) subshells only begin at \(n=3\).
16. Answer: (C) Argon atom (\(\text{Ar}\))
Isoelectronic: \(\text{S}^{2-}\) has \(16 + 2 = 18\) electrons, identical to neutral \(\text{Ar}\) (\(1s^2 2s^2 2p^6 3s^2 3p^6\)).
Total valence electrons \(= 2 + 3 = 5\). Corresponds to the Nitrogen family (Group 15 in IUPAC numbering).
18. Answer: (B) 2s: \([\uparrow\downarrow]\) 2p: \([\uparrow\ ][\uparrow\ ][\uparrow\ ]\)
Hund's Rule: Degenerate \(2p\) orbitals must be singly occupied with parallel spins before any pairing occurs.
Quick Remediation Crosswalk (Test Item Mapping):
Missed Q1–4, 23 (Families/Safety)?
Missed Q5, 9, 10, 17 (Subatomic/Ions)?
Missed Q18, 22, 29–31 (Mass Spec)?
Chemistry Interim Solutions Guide Page 2 of 2 Scoring Rubric & Remediation Crosswalk
