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20 Terms
1
What does the word 'atom' mean in Greek?
Indivisible
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2
What is the significance of the Law of Conservation of Mass?
It states that matter is composed of small, indestructible particles.
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3
Who proposed the Law of Definite Proportions?
Joseph Proust
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4
What does the Law of Multiple Proportions explain?
When two elements form two different compounds, the masses of one element that combine with a fixed mass of the other can be expressed as a ratio of small whole numbers.
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5
What experiment did J.J. Thomson conduct to discover the electron?
He used a cathode ray tube.
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6
What is the charge of an electron?
Negative.
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7
What model did Thomposn propose for the structure of the atom?
The plum-pudding model.
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8
What did Rutherford conclude from his gold foil experiment?
Most of the atom's mass and all of its positive charge are contained in a small core called a nucleus.
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9
What are neutrons and how are they different from protons?
Neutrons have a similar mass to protons but no electrical charge.
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10
How is an element defined?
By the number of protons in its nucleus.
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11
What do isotopes have in common?
The same number of protons but different numbers of neutrons.
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12
What periodic law did Mendeleev establish?
When the elements are arranged in order of increasing mass, certain sets of properties recur periodically.
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13
What group do noble gases belong to?
Group 8A
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14
What are alkali metals?
Group 1A elements that are all reactive metals.
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15
What are cations?
Positively charged ions formed when atoms lose electrons.
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16
What is the mole in chemistry?
A measure containing 6.022 x 10^23 particles.
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17
How are atomic mass and molar mass related?
The molar mass in grams per mole is numerically equal to the atomic mass in amu.
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18
What is the purpose of mass spectrometry?
To separate particles based on the ratio of mass to charge.
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19
Why is Avogadro's number important?
It allows chemists to count particles by weighing them.
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20
What is the equation to calculate atomic mass based on isotopes?
Atomic mass = (fraction of isotope 1 x mass of isotope 1) + (fraction of isotope 2 x mass of isotope 2) + ...
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