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Honors Chemistry > Unit 2: Chapters 4 & 5 > Flashcards

Unit 2: Chapters 4 & 5 Flashcards

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1
Q

What is an atom?

A

An atom is the smallest unit that can exist alone or in combination with other atoms. It comes from the Greek word “Atomon” which means “Indivisible”.

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2
Q

Name the two main areas of an atom.

A

Nucleus and Electron cloud

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3
Q

What is the nucleus?

A

It contains protons (+) and neutrons (0), and it is dense and small.

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4
Q

What is an electron cloud?

A

It contains the electrons(-). It surrounds the nucleus and is mostly empty space; it is arranged in shells or energy levels.

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5
Q

Is an atom itself positively charged, negatively charged, or neutral? Why?

A

An atom itself is neutral because the number of protons (p+) is equal to the number of electrons (e-). The neutrons are neutral and have no effect.

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6
Q

What is an ion?

A

An ion is an atom or molecule in which the total number of electrons does not equal the total number of protons. These particles have a charge.

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7
Q

What is a positively charged ion called?

A

A cation

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8
Q

What is a negatively charged ion called?

A

An anion

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9
Q

Do positively charged ions lose or gain electrons?

A

They lose electrons

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10
Q

Do negatively charged ions lose or gain electrons?

A

They gain electrons

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11
Q

What is an isotope?

A

Isotopes are atoms of the same element with different masses due to a different number of neutrons.

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12
Q

What is the only part of an atom that changes in an isotope?

A

The amount of neutrons

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13
Q

What part of the atom determines what element it is?

A

The protons

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14
Q

What do we measure an atom in?

A

Angstroms 1 A0 = 1 X 10^-10 m

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15
Q

Which is larger the nucleus or the electron cloud?

A

The nucleus is very tiny compared to the electron cloud.

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16
Q

Which two parts of the atom are very similar in mass?

A

Protons and Neutrons

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17
Q

Who was Democritus?

A

He was a Greek thinker who was first to introduce the idea of the atom. (400 BC)

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18
Q

Who was Antoine Lavoisier?

A

He developed the law of Conservation of Mass which stated matter cannot be created nor destroyed. (1782)

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19
Q

Who was Joseph Proust?

A

He developed the Law of Definite Proportions which stated a chemical compound contains the same elements in exactly the same proportions by mass.

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20
Q

What is the Atomic Number?

A

The number of protons in the nucleus of an atom (equal to number of electrons).

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21
Q

What is the Mass Number?

A

The number of protons and neutrons in the nucleus of an atom.

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22
Q

What is the Atomic Weight (Mass)>

A

The average mass of the isotopes

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23
Q

Explain the relation between the mass number and atomic weight.

A

The mass number is just the atomic weight rounded to a whole number.

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24
Q

What is an atomic mass unit (amu)?

A

A special unit for the mass of an atom. It is based off of carbon-12. It is 1/12 the mass of a carbon-12 atom.

25
Q

Who’s was John Dalton?

A

He developed the Law of Multiple Proportions which states that if compounds are composed of the same elements, the masses of the elements can be expressed as ratios of small whole numbers. He also developed the Atomic Theory. (1803)

26
Q

Name the four points of the atomic theory.

A
  1. All matter is composed of extremely small, indivisible particles, called atoms. 2. Atoms of the same element are chemically alike. Atoms of different elements are chemically different. 3. Atoms combine in whole number ratios to form compounds. 4. Atoms are combined, separated, or rearranged in chemical reactions.
27
Q

Who was Joseph Thompson?

A

He used a cathode ray tube to prove there were negative charged particles (electrons) in an atom. This opened the way to the idea that an atom was not just a solid sphere not able to be broken down anymore. (1897)

28
Q

Who was Earnest Rutherford?

A

He conducted a gold foil experiment where he proved that the electron cloud was huge in volume in comparison to the nucleus and the nucleus was extremely dense. (1911)

29
Q

Who was Neils Bohr?

A

He proposed a model of the atom that showed that electrons circled the nucleus of an atom in only allowed orbits or paths. (1913)

30
Q

What is the name of this model?

A

Dalton Model. It was developed in 1803 by John Dalton. He believed that an atom was an indestructable particle with no internal frame. (aka Billiard Ball Model)

31
Q

What is the name of this model?

A

The Thomson Model. It was developed by JJ Thomson in 1897 when he discovered electrons. He believed electrons were embedded in positive charge sphere. (Plum Pudding Model)

32
Q

What is the name of this model?

A

The Rutherford Model. It was developed in 1911 by Ernest Rutherford when he discovered there was a dense, positively charged nucleus. Electrons go around the nucleus.

33
Q

What is the name of this model?

A

The Bohr Model. In 1913, Niels Bohr enhanced Rutherford’s model by having electrons move in a circular orbit at fixed distances from the nucleus.

34
Q

What type of elements gain or lose electrons?

A

Metals lose electrons and NonMetals gain electrons.

35
Q

What is the equation to show how many electrons can fit in a shell maximum?

A

2n2; n= shell number

36
Q

How can electrons orbit according to the Bohr Model?

A

Electrons can only orbit the nucleus in specific, allowed pathways.

37
Q

How do electrons move toward or away from the nucleus?

A

They move toward and away from the nucleus by “steps” or discrete amounts of energy that are released or absorbed.

38
Q

Do electrons have more energy if they are closer or farther away from the nucleus?

A

Electrons have more energy if they are farther away from the nucleus. Those closer to the nucleus have less energy.

39
Q

Where can electrons not exist?

A

Electrons can not exist between energy levels.

40
Q

What is ground state?

A

Ground state is the lowest energy of an atom.

41
Q

What is excited state?

A

Excited state is higher potential energy state.

42
Q

What happens to electrons when energy is absorbed?

A

They move to a higher (more excited) state.

43
Q

What happens to electrons when energy is emitted?

A

Electrons move to a lower state.

44
Q

Who proposed that electrons have a wave nature?

A

Louis de Broglie in 1924

45
Q

Who was Erwin Schrödinger and what did he do?

A

IN 1926, he developed a wave equation for electrons that described their energy values correctly.

46
Q

Who was Werner Heisenberg?

A

He developed his Uncertainty Principle that stated it is impossible to determine simultaniously both the position and velocity of an electron or any other particle in 1927.

47
Q

What did Louis de Broglie, Erwin Schrödinger, and Werner Heisenberg ideas all lead to?

A

The modern quantum theory

48
Q

Name three main ideas of Modern Atomic Theory.

A
  1. Orbitals describe the three dimensional space that electrons occupy.
  2. The location of an electron can only be described by probability.
  3. Orbitals give shape to the atom.
49
Q

What is Quantum Mechanics in its simplest?

A

The “adress” of an electron

50
Q

Name the four ways electrons are identified.

A
  1. Principle (n)
  2. Orbital (l)
  3. Magnetic (ml)
  4. Spin (ms)
51
Q

Name the four quantum numbers.

A
  1. Principle Quantum Number
  2. Orbital Quantum Number
  3. Magnetic Quantum Number
  4. Spin Quantum Number
52
Q

Describe the first Quantum Number.

A
  1. The Principle Quantum Number (n)
  • Indicates the main energy level occupied by the electron (distance from the nucleus)
  • Shell Number
  • Values of *n *can only be positive intergers
53
Q

Describe the 2nd Quantum Number

A
  1. Orbital Quantum Number
  • Indicates the shape of the orbital
    • 3D space where the probabilty of finding the electron is greatest
  • Sublevel of *n *
  • Designated s, p, d, f
54
Q

Describe s, p, d, and f

A
  • S orbital
    • Spherical shaped
    • One orbital
    • Holds two electrons
  • p orbital
    • Peanut or dumbell shaped
    • Three orbitals
    • Holds six electrons
  • d orbital
    • Double peanut shaped
    • Five orbitals
    • Holds ten electrons
  • f orbtial
    • flower shaped
    • seven orbitals
    • holds fourteen electrons
55
Q

Describe the third Quantum Number

A
  1. Magnetic Quantum Number
  • Indicates the orientation of an obital
  • p orbitals have three different orientations (px, py, pz)
56
Q

Describe the fourth Quantum Number

A
  1. Spin Quantum Number
  • Indicates the two spin states of an electron in an orbital
    • Only two electrons in each orbital and they spin in opposite directions
  • Represented by arrows
57
Q

What is the Aufbau (“building up”) principle?

A

An electron occupies the lowest energy possible

58
Q

What is Hund’s rule?

A

Orbitals of equal energy are each occupied by one electron before accepting a second electron.

59
Q

What is the Pauli exclusion principle?

A

No two electrons in the same atom will have the same set of quantum numbers. (no two fans have the same seat)

Honors Chemistry (1 decks)

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