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AP Chemistry > Unit 1: Atomic Structure and Properties > Flashcards

Unit 1: Atomic Structure and Properties Flashcards

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1
Q

What is a mole?

A

A mole is a unit of matter that unifies the different elements.

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2
Q

What is Avogadro’s Number?

A

6.022 x 10^23

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3
Q

Every mole has how many atoms/molecules/formula units?

A

6.022 x 10^23 (Avogadro’s Number)

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4
Q

What is one mole equal to?

A

One mole is equal to the molar mass of the element/compound in grams.

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5
Q

How do you find the molar mass of a compound?

A

The molar mass of a compound can be found by adding the molar masses of the elements in the compound.

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6
Q

What are the 7 diatomic elements?

A

BRINCLHOF
Bromine, Iodine, Nitrogen, Chlorine, Hydrogen, Oxygen, and Fluorine

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7
Q

What is a isotope?

A

An isotope is a version of an element that has a different mass than the original element.

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8
Q

What is mass spectroscopy?

A

Mass Spectroscopy is an analytical tool that shows the relative abundance of each isotope in a sample.

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9
Q

How do you find the mass percent of an element in a compound?

A

The formula is (mass of the element/molar mass) x 100.

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10
Q

What is an empirical formula?

A

An empirical formula is the simplest form of a chemical formula
C6H12O6 -> CH2O

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11
Q

How do you write the electron configuration of Sodium?

A

1s^2 2s^2 2p^6 3s^1

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12
Q

What is orbital notation?

A

Orbital notation represents every electron in an atom with an arrow.

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13
Q

What does Photoelectron Spectroscopy do?

A

Photoelectron Spectroscopy (PES) uses the binding energy of electrons to show the electron configuration of an element.

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14
Q

What is Nuclear Charge?

A

The Nuclear Charge is the number of protons in an element.

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15
Q

Electrons closer to the nucleus have a _______ binding energy.

A

Electrons closer to the nucleus have a greater binding energy.

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16
Q

What is an excited state?

A

An excited state is when an electron moves to a higher energy level.

17
Q

How is an atom in an excited state notated?

A

With an Asterisk
Example: Na*

18
Q

What is Periodicity?

A

Periodicity is a cycle of repeating properties that occur as you move across the periodic table from left to right.

19
Q

What are the 2 things that effect a periodic trend?

A

The change in nuclear charge and shielding effect.

20
Q

What is shielding effect?

A

The outer electrons are repelled by the core electrons, so the nucleus’ effective charge on the outermost electrons is decreased. As a result, the outer electrons are shielded and thus have less grip on the nucleus.

21
Q

What is the effective nuclear charge?

A

The effective nuclear charge is the nuclear charge that valence electrons feel considering the shielding effect.

22
Q

What is Atomic Radius?

A

The distance between the nucleus and the outside of the electron cloud.

23
Q

What is the trend for the Atomic Radius?

A

Atomic Radius increases down and left on the periodic table.

24
Q

What is Electronegitivity?

A

The pull of an atoms nucleus on the electrons of an adjacent atom.

25
Q

What is the trend for Electronegitivity?

A

Electronegativity increases up and right on the periodic table.
Noble Gases have no electronegativity.

26
Q

What is Electron Affinity?

A

The energy released by an atom when it gains an electron.

27
Q

What is the trend for Electron Affinity?

A

Increases up and right on the periodic table.
Noble gases have no electron affinity.
Full and half-full electron sublevels have unexpectedly low electron affinity.

28
Q

What is Ionization Energy?

A

The amount of energy required to remove an electron.

29
Q

What is the trend for Ionization Energy?

A

Increases up and right on the periodic table.
Noble gases have no ionization energy.
Full and half-full electron sublevels have unexpectedly low ionization energy.
Helium has the highest ionization energy.

AP Chemistry (8 decks)

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