Chem Flashcards

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1
Q

What atom model was associated with Neils Bohr’s atomic theory?

A

Planetary model

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2
Q

What atom model was associated with Dalton’s atomic theory?

A

Billiard Ball

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3
Q

What was Dalton’s atomic theory?

A

(1) Elements consist of indivisible small particles (atoms).

(2) All atoms of the same element are identical; different elements have different types of atom.

(3) Atoms can neither be created nor destroyed.

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4
Q

What atom model was associated with J.J. Thompson’s atomic theory?

A

Raisin Bun

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5
Q

What did J.J. Thomson discover?

A

Electrons

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6
Q

What did Ernest Rutherford discover?

A

The nucleus and proposed the existance of protons

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7
Q

What atom model was associated with Neils Bohr’s atomic theory?

A

Planetary Model

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8
Q

What did Neils Bohr propose?

A

That electrons move in circular orbits around the nucleus.

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9
Q

What did James Chadwick discover?

A

Neutrons! (Jimmy Neutron)

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10
Q

What atom model was associated with Schrodinger/de Broglie’s atomic theory?

A

Quantum model

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11
Q

What does the quantum model have thats special about electrons?

A

That electrons have distinct energy levels and the electron cloud.

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12
Q

What are the atoms proportions?

A

Nucleus (protons and neutrons) = most of the weight of the atom

Electrons = most of the volume of the atom

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13
Q

What are isotopes?

A

Atoms that have the same number of protons but a different number of neutrons

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14
Q

What is group 1 on the periodic table?

A

Alkali Metals

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15
Q

What is group 2 on the periodic table?

A

Alkaline Earth Metals

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16
Q

What is group 17 on the periodic table?

A

Halogens

17
Q

What is group 18 on the periodic table

A

Noble (inert) Gases

18
Q

What is special about each group?

A

They share similar chemical properties (reactivity) although intensity changes

19
Q

What is special about periods on the periodic table?

A

They show a pattern in reactivity which changes from left to right

20
Q

What does the group number indicate? (ignoring the “1” in groups 13-18)

A

How many electrons are in the outermost energy level (ignore transition metals)

21
Q

What does the period number indicate?

A

How many levels of electrons there are (ignore transition metals)

22
Q

What does isoelectronic mean?

A

2 or more atoms/ions with the same number of electrons

23
Q

What are cations? How do we name them?

A

positively charged ions (lose electrons) METALS

Just add ION after the metal

24
Q

What are anions? How do we name them?

A

negatively charged ions (gain electrons) NONMETALS

Add IDE after the nonmetal and then ION