EssayFount's chemistry hub offers free step-by-step worked examples across stoichiometry, atomic structure, thermochemistry, kinetics, equilibrium, acid-base chemistry, organic mechanisms, and biochemistry, plus AP Chemistry review and lab report coursework support help. Every example is written or reviewed by credentialed chemistry writers with PhD or Master of Science chemistry credentials so students learn the method behind every answer. This guide on chemistry homework help walks through the rules, examples, and decisions that come up in real student work.
Authored by Dr. Rohan Mehta, PhD Organic Chemistry, with ten years teaching general and organic chemistry. Peer-reviewed by Dr. Naomi Alvarez, PhD Inorganic Chemistry, with twelve years of research and teaching experience. Last reviewed April 2026.
How students use the EssayFount chemistry hub
This hub was built by 64 verified writing experts holding PhD or Master of Science credentials in general, organic, inorganic, biochemistry, or analytical chemistry. Together they compiled 312 fully worked numerical and mechanism problems across the topic lanes below. Students reach the page most often the night before a problem set is due, in the two-week stretch before a midterm or final, and during AP Chemistry review season in March through May.
Every worked problem passes a two-tier review. A subject-matter writer drafts each solution; a second senior chemist verifies the balanced equations, the unit conversions, the curved-arrow mechanism, and the final reported value before publication. Read more about the credential verification process behind every byline on the our writing experts page.
The hub complements rather than replaces a course. Students should still attend lectures, read the assigned chapters in Tro's Chemistry: A Molecular Approach, Brown et al.'s Chemistry: The Central Science, or Clayden, Greeves, and Warren's Organic Chemistry, and attempt problems unaided first. For peer subject support, see our math pillar academic resources, programming pillar essay help, statistics and SPSS pillar, pharmacy and pharmacology pillar, and nursing pillar research papers. For a fully written assignment with model results, see our chemistry writing service and, for a chemistry lab report or research paper, our dissertation chapter help.
Stoichiometry
Stoichiometry uses balanced chemical equations and mole ratios to relate the quantities of reactants and products in a reaction. Every quantitative chemistry problem starts with a balanced equation and a mole conversion; mastering both removes most of the difficulty from later coursework.
Mole concept and Avogadro's number
One mole equals exactly 6.02214076 times ten to the twenty-third entities (Avogadro's number, fixed by the 2019 redefinition of the International System of Units). The molar mass of a compound in grams per mole equals the sum of the atomic weights of its atoms. Conversions between mass, moles, and number of particles follow predictably: divide grams by molar mass to get moles; multiply moles by Avogadro's number to get particle count.
Balancing chemical equations
Balance equations by inspection: count each element on both sides, then adjust coefficients (never subscripts) so element counts match. For combustion of hydrocarbons, balance carbon first, then hydrogen, then oxygen last. For redox reactions in acidic or basic solution, use the half-reaction method: write each half-reaction, balance atoms other than oxygen and hydrogen, balance oxygen with water, balance hydrogen with hydronium (acidic) or hydroxide (basic), balance charge with electrons, then add half-reactions and cancel.
Limiting reagent and percent yield
The limiting reagent is the reactant that runs out first and limits the amount of product formed. Identify it by computing the moles of product each reactant could produce; the smallest value is the theoretical yield, and the reactant that produced it is the limiting reagent. Percent yield equals actual yield divided by theoretical yield, multiplied by 100.
Worked example: find the limiting reagent and theoretical yield
Hydrogen gas reacts with nitrogen gas to form ammonia: 3H two plus N two yields 2NH three. Given 4.0 grams of hydrogen and 28.0 grams of nitrogen, find the limiting reagent and the theoretical yield of ammonia. Convert: 4.0 grams of hydrogen divided by 2.016 grams per mole equals 1.984 moles. 28.0 grams of nitrogen divided by 28.014 grams per mole equals 1.000 mole. Mole ratio test: 1.984 moles of hydrogen times (2 mol ammonia divided by 3 mol hydrogen) equals 1.323 moles of ammonia available from hydrogen. 1.000 mole of nitrogen times (2 mol ammonia divided by 1 mol nitrogen) equals 2.000 moles of ammonia available from nitrogen. Hydrogen produces less ammonia, so hydrogen is the limiting reagent; theoretical yield is 1.323 moles of ammonia, or 22.5 grams.
For deeper dives by topic, follow through to the general chemistry sub-pillar, organic chemistry sub-pillar, and biochemistry sub-pillar.
Atomic structure and periodicity
Atomic structure describes the arrangement of electrons in an atom; periodicity explains how atomic properties change across the periodic table. Both topics anchor the rest of general chemistry, since bonding, reactivity, and physical properties trace back to electron configuration and effective nuclear charge.
Quantum numbers and electron configuration
Four quantum numbers fully specify an electron's state: principal n (shell), angular momentum l (subshell, s p d f), magnetic m sub l (orbital orientation), and spin m sub s (plus or minus one half). The Pauli exclusion principle requires every electron to have a unique quartet. Build electron configurations by filling subshells in the order set by the Aufbau principle (1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p), placing two electrons per orbital with opposite spins.
Periodic trends
Atomic radius decreases left to right across a period and increases down a group. Ionization energy and electronegativity follow the opposite pattern: increase left to right, decrease down a group. Electron affinity is more irregular but generally increases left to right. Effective nuclear charge explains all four trends: greater positive nuclear pull on the outer electrons compresses the atom and makes electron removal harder.
Worked example: write the electron configuration for a transition metal
Iron (Fe, atomic number 26): fill the orbitals through 4s before 3d per the Aufbau order. Configuration: 1s2 2s2 2p6 3s2 3p6 4s2 3d6, abbreviated [Ar] 4s2 3d6. The plus 2 cation (Fe2 plus) loses the 4s electrons first (not the 3d, despite the filling order), giving [Ar] 3d6. The plus 3 cation (Fe3 plus) loses one more electron from 3d, giving the half-filled stable [Ar] 3d5 configuration that explains iron's preference for the plus 3 oxidation state in aqueous chemistry.
Chemical bonding and molecular geometry
Chemical bonding describes how atoms share or transfer electrons to form molecules and ions; molecular geometry describes the three-dimensional arrangement of atoms in those structures. Geometry determines polarity, reactivity, and physical properties like boiling point, so getting it right is foundational.
Lewis structures and formal charge
Draw a Lewis structure in five steps. Count valence electrons (sum across all atoms, add for negative charge, subtract for positive). Place the least-electronegative atom in the center (hydrogen and fluorine never go in the center). Connect atoms with single bonds. Distribute remaining electrons as lone pairs to satisfy octets, starting with the outer atoms. Convert lone pairs to multiple bonds if the central atom lacks an octet. Compute formal charge for each atom: valence electrons minus lone pair electrons minus half the bonding electrons. The best Lewis structure minimizes formal charges.
VSEPR theory and molecular geometry
Valence Shell Electron Pair Repulsion theory predicts molecular geometry from the number of electron domains around the central atom (bonds count as one domain regardless of order, lone pairs count as one domain each). Two domains: linear, 180 degrees. Three: trigonal planar, 120 degrees. Four: tetrahedral, 109.5 degrees. Five: trigonal bipyramidal, 90 and 120 degrees. Six: octahedral, 90 degrees. Lone pairs replace bonded atoms in the geometric framework but still occupy a domain, producing bent, trigonal pyramidal, seesaw, T-shaped, and square pyramidal variants.
Hybridization and molecular orbital theory
Hybridization mixes atomic orbitals on the central atom to produce equivalent hybrid orbitals oriented toward bonded atoms: sp linear, sp2 trigonal planar, sp3 tetrahedral, sp3d trigonal bipyramidal, sp3d2 octahedral. Molecular orbital theory generalizes further by combining atomic orbitals across the entire molecule into bonding and antibonding orbitals, explaining phenomena like the magnetism of molecular oxygen that Lewis and VSEPR cannot.
Worked example: draw the Lewis structure and predict geometry
Sulfur tetrafluoride (SF4): valence electrons equal 6 (sulfur) plus 4 times 7 (fluorines) equals 34. Place sulfur in the center, attach four fluorines with single bonds (uses 8 electrons), distribute the remaining 26 as three lone pairs on each fluorine (24 used) and one lone pair on sulfur (2 used). Sulfur has five electron domains (4 bonds plus 1 lone pair): trigonal bipyramidal electron geometry, seesaw molecular geometry. Bond angles are slightly less than 90 and 120 degrees due to lone pair repulsion.
Thermochemistry and thermodynamics
Thermochemistry studies the heat absorbed or released by chemical reactions; thermodynamics expands the framework to predict whether a reaction is spontaneous. Three state functions carry the analytical load: enthalpy H, entropy S, and Gibbs free energy G.
Enthalpy, entropy, and Gibbs free energy
Enthalpy change delta H equals heat absorbed at constant pressure; negative values indicate exothermic reactions, positive values endothermic. Entropy change delta S equals the change in disorder; positive values indicate increased dispersal of energy or matter. Gibbs free energy change delta G equals delta H minus T times delta S, where T is the temperature in kelvin; negative delta G indicates a thermodynamically spontaneous reaction at that temperature.
Hess's law and standard enthalpies of formation
Hess's law states that the enthalpy change of a reaction equals the sum of enthalpy changes of any steps that, summed, produce the same overall reaction. Standard enthalpies of formation (delta H f standard, in kilojoules per mole) are tabulated for compounds in their standard states; the standard enthalpy of formation of an element in its standard state equals zero by definition. For any reaction, delta H reaction equals the sum of products' enthalpies of formation minus the sum of reactants' enthalpies of formation, weighted by stoichiometric coefficients.
Worked example: calculate Gibbs free energy from enthalpy and entropy
For the reaction 2H two plus O two yields 2H two O at 298 kelvin: delta H equals negative 571.6 kilojoules per mole, delta S equals negative 0.327 kilojoules per mole per kelvin. Compute delta G: delta G equals delta H minus T delta S equals negative 571.6 minus (298 times negative 0.327) equals negative 571.6 plus 97.4 equals negative 474.2 kilojoules per mole. The negative delta G confirms the reaction is spontaneous at room temperature, consistent with the explosive behavior of hydrogen-oxygen mixtures.
Chemical kinetics
Chemical kinetics studies reaction rates and the factors that affect them. Where thermodynamics asks whether a reaction can happen, kinetics asks how fast.
Rate laws and reaction order
A rate law expresses the reaction rate as rate equals k times concentration of A to the m times concentration of B to the n, where k is the rate constant and m and n are the reaction orders in A and B. The overall order is m plus n. Orders are determined experimentally, not from the balanced equation. The method of initial rates compares experimental runs at different starting concentrations to deduce orders.
Arrhenius equation and activation energy
The Arrhenius equation k equals A times e to the negative E sub a divided by RT relates the rate constant to temperature, the pre-exponential factor A, the activation energy E sub a, and the gas constant R. Plotting natural log of k versus one over T gives a straight line with slope negative E sub a divided by R; this is the standard graphical method for determining activation energy from temperature-dependent rate data.
Reaction mechanisms and rate-determining step
A reaction mechanism breaks the overall reaction into elementary steps. The slowest step is the rate-determining step and sets the overall rate law. A proposed mechanism must (1) sum to the overall reaction, (2) be consistent with the experimental rate law, and (3) involve only physically plausible elementary steps.
Worked example: determine reaction order from initial rates
For the reaction A plus B yields C, three experiments yield: trial 1 with [A] equal 0.10, [B] equal 0.10, rate equal 0.020 molar per second. Trial 2 with [A] equal 0.20, [B] equal 0.10, rate equal 0.040. Trial 3 with [A] equal 0.10, [B] equal 0.20, rate equal 0.080. From trials 1 and 2, doubling [A] doubles the rate, so the order in A is 1. From trials 1 and 3, doubling [B] quadruples the rate, so the order in B is 2. The overall rate law: rate equals k times [A] times [B] squared, overall third order.
Chemical equilibrium
Chemical equilibrium occurs when forward and reverse reaction rates equalize and the concentrations of reactants and products remain constant over time. The equilibrium constant K describes the ratio of product to reactant activities at equilibrium and is temperature-dependent.
Equilibrium constant K and reaction quotient Q
For the general reaction aA plus bB equilibrium with cC plus dD, the equilibrium constant K equals concentrations of products to their stoichiometric powers divided by concentrations of reactants to their stoichiometric powers, evaluated at equilibrium. The reaction quotient Q has the same form but is evaluated at any moment. If Q is less than K, the reaction proceeds forward; if Q equals K, the reaction is at equilibrium; if Q is greater than K, the reaction proceeds in reverse.
Le Chatelier's principle
Le Chatelier's principle states that if a system at equilibrium is disturbed, the equilibrium shifts to partially counteract the disturbance. Adding a reactant shifts forward; removing a product shifts forward; increasing pressure on a gas-phase reaction shifts toward the side with fewer moles of gas; increasing temperature shifts toward the endothermic direction. Predict the shift, then quantify with an ICE table.
ICE tables for equilibrium calculations
An ICE table tracks Initial concentrations, Change in concentration during the approach to equilibrium, and Equilibrium concentration. Set up the table with one column per species, one row per phase. Define x as the change in a chosen reference species, then express the other changes as multiples of x using stoichiometry. Substitute the equilibrium row into the K expression and solve for x.
Worked example: ICE table for a weak acid dissociation
For acetic acid (Ka equal 1.8 times ten to the negative 5) at initial concentration 0.10 molar in water: ICE table for CH three COOH equilibrium with H plus and CH three COO minus. Initial: 0.10, 0, 0. Change: minus x, plus x, plus x. Equilibrium: 0.10 minus x, x, x. Ka equals x squared divided by (0.10 minus x). Approximating x as small relative to 0.10, x squared equals 1.8 times ten to the negative 6, so x equals 1.34 times ten to the negative 3 molar. The pH equals negative log of x equals 2.87. Check the approximation: x divided by 0.10 equals 0.0134 or 1.3 percent, well below the 5 percent threshold.
Acid-base chemistry
Acid-base chemistry describes proton transfer between species. Three definition systems coexist: Arrhenius (acids release hydronium in water), Bronsted-Lowry (acids donate protons, bases accept them), and Lewis (acids accept electron pairs, bases donate them). Bronsted-Lowry is the working definition for most homework.
Bronsted-Lowry and Lewis definitions
Under Bronsted-Lowry, every acid has a conjugate base, formed by losing a proton; every base has a conjugate acid, formed by gaining a proton. The Lewis definition extends acid-base behavior to reactions without proton transfer, like the formation of complex ions and many organic reactions involving electrophiles and nucleophiles.
pH, pOH, and pKa
pH equals negative log base ten of hydronium concentration; pOH equals negative log base ten of hydroxide concentration. At 25 degrees Celsius, pH plus pOH equals 14. Strong acids and strong bases dissociate fully; weak acids and weak bases dissociate partially, characterized by Ka or Kb. pKa equals negative log of Ka; lower pKa means a stronger acid. The pKa of a conjugate acid plus the pKb of its conjugate base equals 14.
Buffers and the Henderson-Hasselbalch equation
A buffer resists pH change when small amounts of acid or base are added. The Henderson-Hasselbalch equation, pH equals pKa plus log of conjugate base concentration divided by acid concentration, predicts buffer pH from the conjugate acid-base ratio. Optimal buffering occurs when pH is within plus or minus one of pKa.
Acid-base titrations
A titration adds a titrant of known concentration to an analyte until the equivalence point. The titration curve plots pH versus volume of titrant added; the equivalence point appears as the steepest portion of the curve, and the pH at the equivalence point depends on the strength of the analyte and titrant. Strong acid plus strong base gives pH equal 7 at equivalence; weak acid plus strong base gives pH greater than 7; strong acid plus weak base gives pH less than 7.
Worked example: buffer pH calculation
A buffer contains 0.10 molar acetic acid and 0.20 molar sodium acetate. The pKa of acetic acid is 4.74. Compute the buffer pH: pH equals 4.74 plus log of (0.20 divided by 0.10) equals 4.74 plus log 2 equals 4.74 plus 0.30 equals 5.04. Add 5 millimoles of strong acid (HCl) to one liter of this buffer: the H plus reacts with acetate to form acetic acid. New concentrations: acetic acid 0.105 molar, acetate 0.195 molar. New pH equals 4.74 plus log of (0.195 divided by 0.105) equals 4.74 plus 0.270 equals 5.01. The buffer absorbed the strong acid with negligible pH change.
Organic chemistry help
Organic chemistry is the chemistry of carbon-containing compounds. Two skills carry the entire course: structure (drawing and interpreting molecules in two and three dimensions) and mechanism (predicting how electrons move during reactions). Both reward systematic practice over memorization.
IUPAC nomenclature and functional groups
IUPAC nomenclature names organic compounds by parent chain (the longest continuous carbon chain containing the principal functional group), substituents (alphabetical order, lowest locants), and suffix (denoting the principal functional group). Functional groups include alkanes, alkenes, alkynes, alcohols, ethers, aldehydes, ketones, carboxylic acids, esters, amines, and amides; their priority order determines which becomes the parent and which becomes a substituent.
Stereochemistry, R and S configuration
Stereochemistry distinguishes molecules with the same connectivity but different three-dimensional arrangement. Chirality requires a stereocenter (commonly a carbon with four different substituents). Assign R or S configuration by Cahn-Ingold-Prelog priority: rank the four substituents by atomic number (and then by next-atom comparison if needed), orient the lowest priority away from you, and trace the remaining three from highest to lowest; clockwise is R, counterclockwise is S.
Reaction mechanisms with arrow pushing
Curved arrows show the movement of pairs of electrons during a reaction. A full arrow shows two electrons moving; a half arrow (fishhook) shows one electron moving in radical reactions. The tail of the arrow starts at the electron source (a lone pair, a pi bond, or a sigma bond); the head ends where the new bond forms or where the electrons localize. Mechanism literacy is the single most predictive skill for organic chemistry exam performance.
Substitution and elimination reactions
SN1 substitution proceeds through a carbocation intermediate; first-order kinetics (rate equals k times substrate concentration); favored on tertiary substrates and in polar protic solvents. SN2 substitution proceeds through a single concerted step with backside attack and inversion of stereochemistry; second-order kinetics (rate equals k times substrate times nucleophile); favored on primary substrates and in polar aprotic solvents. E1 and E2 are the elimination counterparts and compete with SN1 and SN2 respectively. The substrate, the nucleophile or base strength, and the solvent together determine which mechanism dominates.
Spectroscopy basics: IR, NMR, mass spectrometry
Infrared spectroscopy identifies functional groups by characteristic absorption bands (carbonyl around 1700 wave numbers, hydroxyl broad band around 3300, nitrogen-hydrogen around 3400). Proton NMR reveals hydrogen environments through chemical shift, multiplicity, and integration. Carbon-13 NMR reveals carbon environments. Mass spectrometry gives the molecular formula and fragmentation pattern. Spectroscopy interpretation is always a best-fit problem; cross-check evidence from multiple spectra before committing to a structure.
Worked example: propose a mechanism for an SN2 reaction
Bromomethane reacts with hydroxide to give methanol and bromide. Mechanism: hydroxide approaches the carbon from the side opposite the bromine. The hydroxide's lone pair forms a new bond to carbon as the carbon-bromine bond breaks heterolytically, with both electrons going to bromine. The transition state has partial bonds to both hydroxide and bromine and an inverted (umbrella-flipped) carbon center. Products: methanol with inverted configuration (relative to the starting bromomethane) and bromide ion.
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Biochemistry homework help
Biochemistry studies the chemical processes within and relating to living organisms, including metabolism, enzyme kinetics, and the structure and function of biomolecules.
Amino acids and protein structure
Twenty standard amino acids share an alpha carbon bearing an amine, a carboxylic acid, a hydrogen, and a side chain that distinguishes them. Side chains classify as nonpolar, polar uncharged, acidic, or basic. Protein primary structure is the amino acid sequence; secondary structure is alpha helices and beta sheets stabilized by backbone hydrogen bonds; tertiary structure is the three-dimensional fold of a single chain; quaternary structure is the assembly of multiple chains.
Enzyme kinetics and Michaelis-Menten
Enzymes accelerate biochemical reactions by lowering activation energy. The Michaelis-Menten equation, v equals V max times [S] divided by K sub M plus [S], describes how reaction velocity v depends on substrate concentration [S], the maximum velocity V max, and the Michaelis constant K sub M (the substrate concentration at which v equals one-half V max). The Lineweaver-Burk plot linearizes the equation and is the classical graphical method for extracting V max and K sub M from experimental data.
Carbohydrate, lipid, and nucleic acid chemistry
Carbohydrates classify as monosaccharides (glucose, fructose), disaccharides (sucrose, lactose), and polysaccharides (starch, glycogen, cellulose). Lipids include triglycerides (energy storage), phospholipids (membrane structure), and steroids (signaling and structure). Nucleic acids (DNA and RNA) consist of nucleotides linked by phosphodiester bonds; the sequence of bases encodes genetic information.
Metabolic pathways overview
Glycolysis converts glucose to pyruvate with a net yield of two ATP and two NADH. The citric acid cycle further oxidizes pyruvate-derived acetyl-CoA, generating NADH, FADH two, and ATP. Oxidative phosphorylation harvests the reducing equivalents from NADH and FADH two through the electron transport chain, generating the bulk of cellular ATP. Connecting individual metabolic steps to their pathway context is the most efficient study strategy for biochemistry exams.
AP Chemistry preparation
AP Chemistry covers nine units defined by the College Board: atomic structure and properties, molecular and ionic compound structure and properties, intermolecular forces and properties, chemical reactions, kinetics, thermodynamics, equilibrium, acids and bases, and applications of thermodynamics.
AP Chemistry units and exam structure
The exam contains 60 multiple-choice questions in 90 minutes and 7 free-response questions (3 long, 4 short) in 105 minutes. Each section is worth 50 percent of the total score. The College Board calculator policy permits a graphing or scientific calculator on all sections. A formula and constants sheet is provided.
Free-response and multiple-choice strategy
Multiple choice rewards process of elimination and recognizing question patterns (acid-base equilibrium, kinetics rate-law deduction, periodic-trend ranking). Free response rewards explicit setup, dimensional analysis, and one-sentence justifications for every numerical answer. Lose one credit for skipping the justification; lose another for forgetting to label the units on a final answer.
Sample free-response walkthrough
Released free-response questions are graded on a multi-point rubric per part. Read the rubric for each released question alongside your written answer and self-grade against the official scoring guide. Repeat with five questions, focus revision on the parts that consistently lose credit, then take a full timed practice section. Expect a one-letter-grade improvement after roughly fifteen hours of structured practice.
Chemistry lab report help
Chemistry lab reports follow a predictable structure regardless of subdiscipline. Knowing the conventions for each section saves time and prevents the rookie errors that lose easy credit.
Lab report sections, abstract through discussion
Standard sections: title, abstract (200 words summarizing purpose, method, key result, and conclusion), introduction (background and hypothesis), materials and methods (reproducible procedure), results (data tables and figures with descriptive captions, no interpretation), discussion (interpretation, error analysis, comparison to literature values), and references. Abstracts are written last; introductions cite background literature and end with a clear hypothesis.
Reporting numerical results with significant figures
Match significant figures to instrument precision. Multiplication and division: result has the same number of significant figures as the least-precise input. Addition and subtraction: result has the same number of decimal places as the least-precise input. Logarithms: the mantissa carries as many significant figures as the original number's significant figures. Always carry one extra digit through intermediate calculations and round only the final reported value.
APA and ACS citation formats for chemistry papers
The American Chemical Society style is standard for chemistry journals; APA seventh edition is common for general-education chemistry courses and interdisciplinary papers. ACS uses superscript numerical citations linked to a numbered reference list; APA uses author-date in-text citations and an alphabetical reference list. Match the style your instructor specifies; never mix the two within a single paper.
Chemistry writing service
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Credentialed chemistry writers, PhD and MS chemists
Every chemistry writer holds a PhD or terminal Master of Science in chemistry, biochemistry, or chemical engineering. Each candidate completes a written test with one mechanism problem and one quantitative equilibrium problem before being approved for student work. Writer credentials are visible on the our writing experts page.
Pricing, per problem and per assignment
Per-problem pricing starts at the low double digits for a single-step stoichiometry or equilibrium question and scales by complexity. Per-assignment pricing covers full problem sets and lab report drafts. Visit our pricing page for the current rate card and turnaround tiers.
How it works
Submit the assignment or lab notebook through the quote form. A chemistry writer accepts the project within an hour during business windows. For lab reports, the writer drafts the discussion section based on your raw data, generates ACS-style or APA-style references, and delivers an editable Word document together with the data tables and figures.
Free chemistry resources
Beyond the worked-example hub, EssayFount publishes free reference resources for self-study.
Periodic table reference
An IUPAC-color-coded periodic table with atomic number, symbol, atomic mass, electron configuration, and electronegativity for each element, formatted for printing.
Reaction mechanism cheat sheets
Curved-arrow templates for the most common organic mechanisms: SN1, SN2, E1, E2, electrophilic aromatic substitution, aldol condensation, Diels-Alder cycloaddition.
Stoichiometry and equilibrium calculators
Try the free stoichiometry, equilibrium, and pH calculators for quick numeric checks during homework.
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