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Science // 3rd Periodic Test > 3rd Periodic Test > Flashcards

3rd Periodic Test Flashcards

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1
Q

The horizontal arrangement in the periodic table.

A

Group

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2
Q

A positively charged subatomic particle.

A

Proton

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3
Q

Describes the spin of an electron in an orbital.

A

Spin Quantum Number

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4
Q

A particle smaller than an atom in which scientists used experimental observations to establish its existence.

A

Subatomic particle

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5
Q

This is equivalent to the number of protons (and electrons, if there is no charge).

A

Atomic Number

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6
Q

He realized you can arrange the elements using atomic number rather than atomic mass.

A

Henry Moseley

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7
Q

He improved the model of Ernest Rutherford

A

Niels Bohr

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8
Q

Specifies the energy of an electron and the size of the orbital and its distance away from the nucleus.

A

Principal Quantum Number

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9
Q

The particles vibrate in a fixed position.

A

Solid

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10
Q

He created the Telluric screw.

A

Alexander Béguyer de Chancourtois

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11
Q

Shape of the sublevel in each energy level.

A

Angular Quantum Number

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12
Q

Its molecules are slightly loose and is not easily compressed.

A

Liquid

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13
Q

He discovered neutrons.

A

James Chadwick

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14
Q

He called his atomic model the planetary model.

A

Niels Bohr

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15
Q

This rule states that no two electrons can have exactly the same amount of quantum numbers.

A

Pauli Exclusion

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16
Q

In which directions does atomic size increase?

A

It increases from right to left and up to down.

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17
Q

Liquid to solid…

A

Freezing

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18
Q

It has no definite shape and definite volume.

A

Liquid

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19
Q

First to discover electrons, he used his cathode ray tube experiment.

A

J.J Thomson

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20
Q

The person who discovered transuranic elements (actinide and lanthanide).

A

Glenn Seaborg

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21
Q

It has definite shape and definite volume.

A

Solid

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22
Q

What is the limit for the p orbital?

A

6 electrons

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23
Q

Its molecules can freely move and it is easily compressible.

A

Gas

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24
Q

He concluded that the atomic mass of the middle is the average atomic mass of the 2 elements.

A

Johann Dobereiner

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25
Q

An unstable atom that either gains or loses electrons.

A

Ion

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26
Q

It is a value that is used when describing the energy levels of electrons in atoms.

A

Quantum Numbers

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27
Q

Democritus’ ideas were not widely accepted as they were opposed by him.

A

Aristotle

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28
Q

It measures the size of the atoms.

A

Atomic Radius

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29
Q

The ability for elements to attract valence electrons.

A

Electronegativity

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30
Q

The vertical arrangement of the periodic table.

A

Series

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31
Q

Believed that matter was made of four natural elements.

A

Aristotle

32
Q

What is formed when an ion gains electrons?

A

Anion

33
Q

Used to show the distribution of electrons in each energy level located in various locations or orbitals.

A

Electron Configuration

34
Q

Published his own arrangement based on increasing atomic mass similar to that of Mendeleev.

A

Lothar Meyer

35
Q

The smallest particle of matter, the building block.

A

Atom

36
Q

Solid to liquid…

A

Melting

37
Q

What is the limit for the f orbital?

A

14 electrons

38
Q

A negatively charged subatomic particle.

A

Electron

39
Q

The representation of what an atom could look like based on observations and scientific evidence.

A

Atomic Model

40
Q

What is formed when an ion loses electrons?

A

Cation

41
Q

A subatomic particle with no charge.

A

Neutron

42
Q

Solid to gas…

A

Sublimation

43
Q

He used Heisenburg’s uncertainty principle to come up with the Electron Cloud Model.

A

Erwin Schrödinger

44
Q

He was the person who revised the periodic law.

A

Henry Moseley

45
Q

Proposed that elements can be arranged using their atomic mass. This may be observed at a regular interval every after the 7th element; this is called the law of octaves.

A

John Newlands

46
Q

This rule states that the very orbital of the same energy must be singly occupied with one electron before any orbital is double occupied.

A

Hund’s rule

47
Q

Describes the orientation of the orbital in the space around the nucleus.

A

Magnetic Quantum Number

48
Q

What is the limit for the d orbital?

A

10 electrons

49
Q

He then arranged the elements by increasing atomic mass, he was also the person who noticed a pattern when arranged horizontally.

A

Dmitri Mendeleev

50
Q

In which direction does Ionization energy, electronegativity, and electron affinity increase?

A

It increases from left to right and bottom to top

51
Q

The vertical arrangement of the periodic table.

A

Series

52
Q

The particles move quickly in all directions.

A

Liquid

53
Q

Whose ideas are these?

  • Atoms are tiny invisible particles.
  • Atoms of an element are all the same.
  • The atoms of different elements vary from one another.
  • Atoms form compounds when combined.
A

John Dalton

54
Q

Amount of energy required to remove an electron from a neutral atom in its gaseous phase.

A

Ionization Energy

55
Q

What is the limit for the s orbital?

A

2 electrons

56
Q

Its molecules are tightly packed an hard to compress.

A

Solid

57
Q

Liquid to gas…

A

Evaporation / Vaporization

58
Q

He created the solid sphere/billiard ball model.

A

John Dalton

59
Q

The particles move quickly in all directions with electric charge.

A

Gas

60
Q

He first attempted to group the elements by threes based on their similar properties. (Law of Triads)

A

Johann Dobereiner

61
Q

Liquid to gas…

A

Deposition

62
Q

Elements that have the same atomic number and number of protons but different number of neutrons.

A

Isotopes

63
Q

He began writing a book named The Principles of Chemistry.

A

Dmitri Mendeleev

64
Q

Pictorial representations of the electrons in an atom.

A

Orbital Diagrams

65
Q

It is the ability of an atom to accept an electron.

A

Electron Affinity

66
Q

It has no definite shape and no definite volume.

A

Gas

67
Q

He thought if you take a piece of matter and keep dividing it, you will come to the point where it cannot be divided anymore.

A

Democritus

68
Q

Whose ideas are these?

  • All things are composed of atomos, which are too small to be seen by the naked eye and cannot be broken down.
  • There are empty spaces between these inner structures of matter.
  • Matter is made of solid particles.
  • Matter has a uniform structure all throughout.
  • Matter varies in shape, size, and weight.
A

Democritus

69
Q

This rule states that the lower energy orbital should be filled first before the next higher energy orbital.

A

Aufbau Principle

70
Q

His atomic model is the plum pudding model.

A

J.J Thomson

71
Q

He determined the atomic number of each known element at that time.

A

Henry Moseley

72
Q

The first scientist to recognize the interval between the elements when they are arranged according to their atomic mass.

A

Alexander Béguyer de Chancourtois

73
Q

His atomic model is the nuclear model.

A

Ernest Rutherford

74
Q

Gas to liquid…

A

Condensation

75
Q

First person to use the term “atom.”

A

Democritus

Science // 3rd Periodic Test (1 decks)

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