chem unit 4

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unit 4 chemistry honors vocabulary + key ideas

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28 Terms

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nuclear model

contains positively charged nucleus (no distinct protons) and electrons. most of the atom is empty space. RUTHERFORD

<p>contains positively charged nucleus (no distinct protons) and electrons. most of the atom is empty space. RUTHERFORD</p>
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solid sphere model

cannot be divided up into smaller parts. DALTON

<p>cannot be divided up into smaller parts. DALTON</p>
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proton model

nucleus consists of protons and electrons, which circle the nucleus — similar to nuclear model. CHADWICK and RUTHERFORD

<p><strong>nucleus consists of protons</strong> and electrons, which circle the nucleus — similar to nuclear model. CHADWICK and RUTHERFORD</p>
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plum pudding model

positive fluid, no nucleus, electrons scattered throughout. THOMSON

<p>positive fluid, no nucleus, electrons scattered throughout. THOMSON</p>
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solar system model

nucleus at center (no distinct protons), electrons circle it at specified orbits. different distances from nucleus. BOHR

<p>nucleus at center (no distinct protons), electrons circle it at specified orbits. different distances from nucleus. BOHR </p>
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who discovered electrons?

thomson

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who discovered protons?

rutherford

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who discovered the nucleus?

rutherford, did NOT know about neutrons

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who discovered neutrons?

rutherford / chadwick

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how were electrons discovered?

cathode ray experiment (thomson)

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how was the nucleus discovered?

gold foil experiment (rutherford)

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how were neutrons discovered?

beryllium / boron / lithium sheet experiment (chadwick)

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how were protons discovered?

scintillation detectors (in progress)

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law of the conservation of mass

matter is neither created nor destroyed, just converted in some way

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dalton’s atomic theory

- matter is made up of small particles called atoms

- atoms are indivisible and indestructible

- atoms of a particular element are identical in size, mass, and chemical properties

- atoms of other elements differ from each other

- different atoms combine in simple whole-number ratios to form compounds

- chemical reaction: atoms are separated, combined, and rearranged

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isotope

same element: same number of protons but different number of neutrons in the nucleus

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mass number

total number of neutrons and protons

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atomic number

number of protons

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atomic mass

similar to mass number, but includes the electrons, so it is an approximation of an atom’s total mass

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radioactive decay

emission of energy in the form of ionizing radiation

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fusion

joining of 2 nuclei to form a larger nucleus. accompanied by a large amount of energy (e.g. hydrogen bombs)

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fission

separation of a nucleus into 2 smaller nuclei. accompanied by a large amount of energy

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electron, proton, neutron, gamma, beta, alpha symbols

e-, p+, no, γ, β, α (gamma and alpha are different)

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beta decay (particles)

electron is emitted from a radioactive nucleus (neutron becomes proton, gives off electron; when writing an equation with β-, atomic # gains a proton. with β+, atomic # loses a proton.) negative charge, no mass

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alpha decay (particles)

2 protons and 2 neutrons produced during alpha decay. 2 protons, 4 atomic mass

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gamma radiation / particles

emitted from a radioactive nucleus. no charge, no mass

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nuclear chain reaction

a series of reactions following fission, where the emitted neutrons can cause additional fission reactions.

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average atomic mass of an isotope

1. change percent of abundance into decimal (divide by 100)

2. multiply by atomic mass

3. add together to get the average.

use % of abundance and mass number/actual mass