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Atomic Theory: History and Principles

Atomic Theory: History and Principles

Explore the evolution of atomic theory from ancient philosophical roots to modern scientific understanding. Study Dalton's postulates, Thomson's discovery of the electron, and Rutherford's nuclear model. Understand how our view of the atom has changed over time.

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Atomic Theory: History and Principles

Quiz • 20 Questions

Atomic Theory: History and Principles - Flashcards

Flashcards • 20 Cards

Study Notes

5 min • Summary

Materials

List of Questions20 questions
  1. Question 1
    • Dalton's theory stated all atoms of an element have identical mass, whereas modern understanding acknowledges isotopes.
    • Dalton proposed that atoms are divisible, while modern theory states atoms are indivisible.
    • Dalton included the concept of electron orbitals, while modern theory focuses on fixed electron paths.
    • Dalton’s atomic theory proposed compounds are formed by the changing of elements, which is still correct today.
  2. Question 2
    • The concept of specific energy levels or shells in which electrons orbit the nucleus.
    • The understanding that atoms are indivisible and indestructible particles that form mass and matter.
    • The existence of electrons with negative charge evenly distributed within the atom.
    • The presence of a small, dense, positively charged nucleus at the center of the atom.
  3. Question 3
    • By discovering neutrons and incorporating them into the structure within the nucleus of the atom.
    • By incorporating quantum theory to suggest that electrons orbit the nucleus in specific energy levels.
    • By proposing that atoms are mostly empty space with electrons orbiting a positive nucleus.
    • By describing electrons existing in probability regions called orbitals around the nucleus.
  4. Question 4
    • Isotopes are atoms of the same element, thus having the same atomic number but different numbers of neutrons.
    • Isotopes of an element have the same mass number but different atomic numbers.
    • The atomic number is the total number of protons and neutrons in the nucleus.
    • Atoms with the same number of neutrons but different numbers of protons are isotopes.
  5. Question 5
    • Carbon's ability to form stable covalent bonds with itself and other elements leads to a vast diversity of organic compounds.
    • Carbon’s single valence electron allows it to bond and create very durable molecules.
    • Carbon can only bond with hydrogen, forming a limited number of organic compounds.
    • Carbon's ionic bonding nature allows it to create strong crystal lattices, essential for organic structures.
  6. Question 6
    • Alkenes contain one or more carbon-carbon double bonds, while alkynes contain one or more carbon-carbon triple bonds.
    • Alkenes contain triple bonds, while alkynes contain single bonds.
    • Alkenes are cyclic hydrocarbons, while alkynes are linear hydrocarbons.
    • Alkenes contain only single bonds, while alkynes contain only double bonds.
  7. Question 7
    • They contain one or more benzene rings with alternating single and double bonds.
    • They contain only single bonds between carbon atoms in a long chain.
    • They are saturated hydrocarbons with the general formula CₙH₂ₙ₊₂.
    • They consist of carbon and hydrogen atoms arranged in a tetrahedral structure.
  8. Question 8
    • Carboxyl group (-COOH)
    • Carbonyl group (C=O)
    • Amino group (-NH₂)
    • Hydroxyl group (-OH)
  9. Question 9
    • Aldehydes contain a nitrogen atom bonded to a carbonyl group; ketones contain an oxygen atom.
    • Aldehydes have a carbonyl group bonded to two carbon atoms; ketones have it bonded to one carbon and one hydrogen atom.
    • Aldehydes contain a carboxyl group, while ketones contain a hydroxyl group.
    • Aldehydes have a carbonyl group bonded to at least one hydrogen atom; ketones have it bonded to two carbon atoms.
  10. Question 10
    • Structural isomers have the same spatial arrangement but different bonding arrangements, while stereoisomers have different molecular formulas.
    • Structural isomers have different bonding arrangements, while stereoisomers have the same bonding arrangement but different spatial arrangements.
    • Structural isomers have the same bonding arrangement but different spatial arrangements, while stereoisomers have different bonding arrangements.
    • Structural isomers are non-superimposable mirror images, while stereoisomers are identical in every aspect.
  11. Question 11
    • The color of copper being reddish-brown.
    • The density of aluminum being 2.7 g/cm³.
    • The melting point of ice being 0°C.
    • The flammability of ethanol.
  12. Question 12
    • Homogeneous mixtures are composed of elements, while heterogeneous mixtures are composed of compounds.
    • Homogeneous mixtures have a uniform composition throughout, while heterogeneous mixtures have a non-uniform composition.
    • Homogeneous mixtures can be easily separated by physical means, while heterogeneous mixtures require chemical reactions for separation.
    • Homogeneous mixtures are always solids; heterogeneous mixtures are always liquids.
  13. Question 13
    • 0.0045 m
    • 450 m
    • 450.0 m
    • 0.450 m
  14. Question 14
    • Precise but not accurate
    • Accurate but not precise
    • Accurate and precise
    • Neither accurate nor precise
  15. Question 15
    • 2
    • 1
    • 4
    • 3
  16. Question 16
    • Gas
    • Solid
    • Liquid
    • Plasma
  17. Question 17
    • Mass
    • Color
    • Density
    • Temperature
  18. Question 18
    • 20.0 L
    • 5.0 L
    • 10.0 L
    • 15.0 L
  19. Question 19
    • $5.0 \text{ inches} - 2.54 \text{ cm}$
    • $5.0 \text{ inches} + 2.54 \text{ cm}$
    • $5.0 \text{ inches} \times \frac{2.54 \text{ cm}}{1 \text{ inch}}$
    • $5.0 \text{ inches} \times \frac{1 \text{ inch}}{2.54 \text{ cm}}$
  20. Question 20
    • 250.0 g/cm³
    • 2.50 g/cm³
    • 35.0 g/cm³
    • 0.40 g/cm³
List of Flashcards20 flashcards
  1. Card 1
    HintIt describes the fundamental building blocks of matter.Memory TipAtoms make up everything
  2. Card 2
    HintThink of the chemist who laid the groundwork for atomic theory.Memory TipDalton: First modern atomic ideas
  3. Card 3
    HintHe found the negatively charged particle.Memory TipThomson: Electron and 'plum pudding'
  4. Card 4
    HintThink of the experiment involving gold foil and particles.Memory TipRutherford: Nucleus and gold foil
  5. Card 5
    HintHis model introduced electron shells.Memory TipBohr: Quantum energy shells
  6. Card 6
    HintIt's like an element's ID number.Memory TipZ for identity
  7. Card 7
    HintThey are 'cousins' of the same element.Memory TipIso-topes: Same element, different neutrons
  8. Card 8
    HintIt's all about the element that forms many complex molecules.Memory TipCarbon is king
  9. Card 9
    HintTheir names tell you what elements they contain.Memory TipHydro-carbon: H & C
  10. Card 10
    HintThey have the simplest carbon-carbon bonding.Memory TipAlkanes: All single bonds
  11. Card 11
    HintThey have at least one 'double' feature.Memory TipAlkenes: Eat that double bond
  12. Card 12
    HintThey have the strongest carbon-carbon bond type.Memory TipAlkynes: Triple bond power
  13. Card 13
    HintThey determine how a molecule 'behaves' chemically.Memory TipFunction = reaction part
  14. Card 14
    HintThink of them as having the same 'ingredients' but different 'recipes'.Memory TipIso-mers: Same formula, different structure
  15. Card 15
    HintIt's what everything around you is made of.Memory TipMatter has mass and space
  16. Card 16
    HintThey are the fundamental building blocks on the periodic table.Memory TipElements are fundamental
  17. Card 17
    HintThey are made when elements join up.Memory TipCom-pounds are combined
  18. Card 18
    HintThink of hitting the bullseye on a target.Memory TipAccuracy: A for actual
  19. Card 19
    HintThink of consistently hitting the same spot on a target, even if it's not the bullseye.Memory TipPrecision: P for repeatable
  20. Card 20
    HintThey indicate the reliability of a measurement.Memory TipSig Figs: Reliable numbers

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