chap 2 chem test Flashcards

1
Q

What subatomic atoms equal to each other?

A

electrons = protons

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2
Q

What are isotopes?

A

isotopes have the same number of protons but different number of neutrons

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3
Q

What is core charge?

A

The core charge of an atom is a measure of the attractive force felt by the valence shell electrons towards the nucleus.

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4
Q

How do you find core charge?

A

number of protons in the nucleus - number of total inner shell electrons

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5
Q

What are critical elements?

A

Elements that are heavily relied on for industry & society in areas such as renewable energy, food suppply, electronics and medicine. E.G: platinum used as a catalyst

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6
Q

Compare between the Schrodinger vs Bohr

A

Bohr regarded electrons as particles that travel along a defined path in circular orbits.
Shrodinger’s response is that electrons behave as waves and occupy a three dimensional space around the nucleus.

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7
Q

Why does 4s come before 3d?

A

4s electrons are farther and more loosely held by the nucleus as compared to 3d.

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8
Q

What is the trend for reactivity of metals in the periodic table?

A

increases down a group
decreases across a period

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9
Q

What is the trend of reactivity in non-metals in the periodic table?

A

decreases down a group (greater number of shells making it harder to attract electrons)
increases across the period

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10
Q

What is electronegativity and atomic radius?

A

Electronegativity is the ability of an atom to attract electrons toward itself
Atomic radius is a measurement used for the size of atoms

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11
Q

What is the trend of electronegativity in the periodic table?

A

Decreases down a group (The valence electrons are less strongly attracted to the nucleus as they are further from the nucleus)
Increases left to right across a period (The valence electrons become more strongly attraced to the nucleus as the core charge increases).

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12
Q

What is the trend in atomic radius in the periodic table?

A

Increases down a group (The number of shells increases)
Decreases left to right across a period (Core charge increases)

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13
Q

What is the trend in ionisation energy in the periodic table?

A

Decreases down a group (The valence electrons are less attracted to the nucleus as they are further from the nucleus)
Increases left to right across a group (The core charge increases)

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14
Q

What is the spdf of the schrodinger model?

A

s = 2
p = 6
d = 10
f = 14

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