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Chemistry > Unit 3 > Flashcards

Unit 3 Flashcards

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1
Q

What is Atomic Radius?

A

½ distance between adjacent nuclei
generally this is considered the “size” of an atom

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2
Q

What unit is Atomic Radius measured in?

A

pm

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3
Q

Does Atomic Radius increase or decrease as you go down a group (up and down)?

A

`It increases

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4
Q

Why does the Atomic Radius increase as you go down a group?

A

going down a group, each atom has:​

(1) more energy levels​

(2) greater shielding effect

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5
Q

Does Atomic Radius increase or decrease as you go across a period (left to right)?

A

It decreases

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6
Q

Why are electrons attracted to the nucleus?

A

electrons are attracted to the nucleus due to opposite electrostatic charge

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7
Q

Why does Atomic Radius decrease as it travels across periods?

A

going across a period the number of protons increases, so the electrons are “pulled” closer to the nucleus

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8
Q

What is Ionization Energy?

A

the energy required to excite an electron to the point it is removed from the atom

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9
Q

What is 1st Ionization Energy?

A

energy required to remove one electron​

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10
Q

Does 1st Ionization Energy increase or decrease across a period?

A

1st IE increases across a period

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11
Q

How many groups are there?

A

18

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12
Q

How many periods are there?

A

7

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13
Q

Does 1st Ionization Energy increase or decrease down a group?

A

1st IE decreases down a group

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14
Q

Why does 1st ionization increase across a period?

A

1st IE ↑ across a period because . . .​

the nucleus has more protons​

the e1- that is removed is closer to the nucleus

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15
Q

Why does 1st ionization energy decrease as it goes down a group?

A

1st IE ↓ down a group because . . .​

the atoms have more energy levels, so the e1- is further from the nucleus​

the atoms have more shielding effect which repels the e1- , reducing the energy required to remove it​

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16
Q

What is Ionic Radius?

A

Metal atoms tend to lose electrons

Non-metal atoms are more likely to gain electrons

17
Q

What is Electronegativity?

A

The ability of an atom to attract electrons in a chemical bond

18
Q

Why does Electronegativity increase across a period?

A

Electronegativity increases across a period because . . .​

​

–the nucleus has more protons​

​

–electrons are more strongly attracted when they are closer to the nucleus​

19
Q

Why does Electronegativity decrease down a group?

A

Electronegativity decreases down a group because . . .​

the atoms have more energy levels, so the electrons are further from the nucleus​

the atoms have more shielding effect which repels the electrons, reducing the electronegativity “pull” or attraction​

20
Q

What is the the highest electronegativity element?

A

Highest electronegativity element is fluorine (F) = 4.0

21
Q

What is the lowest electronegativity element?

A

Lowest electronegativity element is francium (Fr) = 0.7

22
Q

What are quantum numbers?

A

The allowed energy states of atoms and molecules can be described by sets of numbers

23
Q

Light is both a _____ and _______

A

Light is both a particle and a wave

24
Q

Quanta (light described as a bundle of energy) of light are often called _______

A

Photons

25
Q

What is the HEISENBERG UNCERTAINTY PRINCIPLE​?

A

States that it is impossible to simultaneously determine both the momentum and the position of an electron.​

​Thus, we speak of the probability of finding an electron within a specified area of space around the nucleus. An orbital is now defined as an area where there is a 90% probability of finding an electron.

26
Q

Who was and what was Erwin Schrödinger’s contribution to The Quantum Mechanical Model​?

A

Austrian physicist Erwin Schrödinger (1887–1961) treated the electron as a wave.

The modern description of the electrons in atoms, the quantum mechanical model, comes from the mathematical solutions to the Schrödinger equation.​

27
Q

What is the The Quantum Mechanical Model​?

A

The probability of finding an electron within a certain volume of space surrounding the nucleus can be represented as a fuzzy cloud.

28
Q

What are the 4 quantum numbers?

A

The Principal Quantum Number​, Azimuthal Quantum Number​, Magnetic Quantum Number, SPIN OF THE ELECTRON.

29
Q

What is the The Principal Quantum Number​?

A

Indicates the main energy level occupied by an electron.

  • represented by n
    -as n goes further from the nucleus the electrons energy increases
30
Q

What is the Azimuthal Quantum Number​?

A

Represents the sublevel of an electron.

-Represented by the letter l
- s,p,d,f

31
Q

What is the Magnetic Quantum Number?

A

Represents the orbital of the electron

-Represented by the symbol Ml

32
Q

What is an orbital?

A

An orbital is an area where you can find a maximum of 2 electrons and is represented by a ​box (electron confiruation chart boxes)

33
Q

What is the Spin of the Electron?

A

Describes whether the electron is spinning clockwise or counterclockwise (behavior of the electron)

-Represented by the symbol Ms
-clockwise spin = up arrow
-counterclockwise = down arrow

34
Q

What is the Aufbau Principle?

A

According to the aufbau principle, electrons occupy the orbitals of lowest energy first.

35
Q

What is the Pauli Exclusion Principle?

A

According to the Pauli exclusion principle, an atomic orbital may describe at most two electrons. To occupy the same orbital, two electrons must have OPPOSITE SPINS; that is, the electron spins must be paired.

36
Q

What is Hund’s Rule​?

A

Hund’s rule states that when electrons occupy orbitals of the same energy, one electron enters each orbital until all contain 1 electron of parallel spin. Once each orbital contains 1 electron, then electrons of opposite spins are filled.

37
Q

What are the types of Electromagnetic Radiation?

A

Gamma rays, X rays, Ultra-violet, Inferred, Microwaves, Radio frequency

(frequency high to low)

38
Q

What is the Periodic Law?

A

a law stating that the elements, when listed in order of their atomic numbers (originally, atomic weights), fall into recurring groups, so that elements with similar properties occur at regular intervals.

39
Q

Who is Mendeleev and what did he do?

A

He came up with the Periodic Law. (arranged elements into periods and groups)

Chemistry (8 decks)

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