Comprehensive Chemistry Flashcards: Elements, Ions, and Bonding Types

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200 Terms

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Chemistry

Study of matter and its changes.

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Matter

Anything with mass and volume.

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Scientific Method

Observation → Hypothesis → Experiment → Theory (explains why) → Law (describes what).

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Quantitative vs. Qualitative

Numerical vs. descriptive data.

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SI Base Units

Length (m), Mass (kg), Time (s), Temp (K), Amount (mol), Current (A), Luminous Intensity (cd).

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SI Prefixes

tera (10¹²), mega (10⁶), kilo (10³), deci (10⁻¹), centi (10⁻²), milli (10⁻³), micro (10⁻⁶), nano (10⁻⁹), pico (10⁻¹²).

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Accuracy vs. Precision

Accuracy = closeness to true value; Precision = reproducibility.

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Error Types

Random (affects precision); Systematic (affects accuracy).

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Significant Figures

Rules for counting and using sig figs; exact numbers have infinite sig figs.

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Dimensional Analysis

Converting units systematically.

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Temperature Conversion

°C = (°F − 32) × 5/9; K = °C + 273.15.

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Solid

fixed shape, volume; not compressible.

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Liquid

fixed volume, takes shape; slightly compressible.

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Gas

no fixed shape or volume; compressible.

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Pure substances

elements or compounds.

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Mixtures

homogeneous (uniform) or heterogeneous (non-uniform).

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Physical vs. Chemical Changes

Physical = no new substance; Chemical = new substance formed.

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Conservation of Mass (Lavoisier)

Matter is neither created nor destroyed.

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Definite Proportions (Proust)

Compounds have constant composition.

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Multiple Proportions (Dalton)

Elements combine in small whole-number ratios.

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Dalton's Atomic Theory

Atoms are indivisible; all atoms of an element are identical; atoms combine in fixed ratios.

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Proton

+1 charge, mass ≈ 1 amu, in nucleus.

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Neutron

0 charge, mass ≈ 1 amu, in nucleus.

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Electron

−1 charge, negligible mass, outside nucleus.

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Atomic Number (Z)

Number of protons; identifies element.

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Mass Number (A)

Protons + neutrons.

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Isotopes

Same Z, different A (different neutrons).

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Periodic Table Groups

Metals, nonmetals, metalloids. Alkali metals (Group 1), Alkaline earth metals (2), Halogens (17), Noble gases (18).

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First 36 elements

H, He, Li, Be, B, C, N, O, F, Ne, Na, Mg, Al, Si, P, S, Cl, Ar, K, Ca, Sc, Ti, V, Cr, Mn, Fe, Co, Ni, Cu, Zn, Ga, Ge, As, Se, Br, Kr.

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Type I Ionic

Fixed cation charge (no Roman numerals). Example: NaCl = sodium chloride.

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Type II Ionic

Variable cation charge (Roman numerals). Example: FeCl₃ = iron(III) chloride.

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Type III Covalent

Prefixes for number of atoms (mono-, di-, tri-, etc.). Example: CO₂ = carbon dioxide.

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Monatomic Anions (-ide endings)

O²⁻ oxide, S²⁻ sulfide, N³⁻ nitride, F⁻ fluoride, Cl⁻ chloride, Br⁻ bromide, I⁻ iodide.

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Polyatomic Ions

CO₃²⁻ carbonate, NO₃⁻ nitrate, SO₄²⁻ sulfate, PO₄³⁻ phosphate. NO₂⁻ nitrite, SO₃²⁻ sulfite, PO₃³⁻ phosphite. CN⁻ cyanide, OH⁻ hydroxide, NH₄⁺ ammonium, C₂H₃O₂⁻ acetate.

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Other Important Ions

CrO₄²⁻ chromate, Cr₂O₇²⁻ dichromate, MnO₄⁻ permanganate. ClO₄⁻ perchlorate, ClO₃⁻ chlorate, ClO₂⁻ chlorite, ClO⁻ hypochlorite (and Br, I analogues).

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Hydrogen Variants

HSO₄⁻ bisulfate, HCO₃⁻ bicarbonate, HPO₄²⁻ hydrogen phosphate, H₂PO₄⁻ dihydrogen phosphate.

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H

Hydrogen

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He

Helium

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Li

Lithium

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Be

Beryllium

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B

Boron

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C

Carbon

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N

Nitrogen

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O

Oxygen

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F

Fluorine

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Ne

Neon

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Na

Sodium

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Mg

Magnesium

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Al

Aluminum

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Si

Silicon

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P

Phosphorus

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S

Sulfur

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Cl

Chlorine

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Ar

Argon

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K

Potassium

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Ca

Calcium

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Sc

Scandium

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Ti

Titanium

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V

Vanadium

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Cr

Chromium

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Mn

Manganese

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Fe

Iron

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Co

Cobalt

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Ni

Nickel

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Cu

Copper

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Zn

Zinc

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Ga

Gallium

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Ge

Germanium

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As

Arsenic

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Se

Selenium

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Br

Bromine

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Kr

Krypton

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Li⁺

Lithium ion

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Na⁺

Sodium ion

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K⁺

Potassium ion

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Rb⁺

Rubidium ion

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Cs⁺

Cesium ion

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Fr⁺

Francium ion

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Be²⁺

Beryllium ion

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Mg²⁺

Magnesium ion

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Ca²⁺

Calcium ion

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Sr²⁺

Strontium ion

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Ba²⁺

Barium ion

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Ra²⁺

Radium ion

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Al³⁺

Aluminum ion

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Zn²⁺

Zinc ion

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Ag⁺

Silver ion

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Cu⁺

Copper(I) ion

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Cu²⁺

Copper(II) ion

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Fe²⁺

Iron(II) ion (ferrous)

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Fe³⁺

Iron(III) ion (ferric)

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Pb²⁺

Lead(II) ion

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Pb⁴⁺

Lead(IV) ion

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Sn²⁺

Tin(II) ion

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Sn⁴⁺

Tin(IV) ion

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H⁻

Hydride

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F⁻

Fluoride

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Cl⁻

Chloride

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Br⁻

Bromide

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I⁻

Iodide