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Freshman Science > Periodic Table Trends and Scientists > Flashcards

Periodic Table Trends and Scientists Flashcards

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1
Q

Who was the first to determine metallic oxides?

A

Alexandre Emile De Chancourtois

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2
Q

Who believed the best way to show the periodic table was to arrange it in a cylinder?

A

Alexandre Emile de Chancourtois, John Newlands, and Glenn T. Seaborg

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3
Q

Who was the first to use chemical characteristics to help arrange the periodic table?

A

Alexandre Emile de Chancourtois

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4
Q

Who used relative atomic mass?

A

Alexandre Emile de Chancourtois and John Newlands

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5
Q

Who arranged the periodic table according to octets like in a musical scale based on both physical and chemical characteristics?

A

John Newlands

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6
Q

Who used physical properties, chemical properties, and relative atomic mass to arrange the periodic table?

A

Julius Lothar Meyer and Dmitri Mendeleev

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7
Q

Whose periodic table had spaces for undiscovered elements?

A

Julius Lothar Meyer and Dmitri Mendeleev

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8
Q

Who believed the best way to arrange the periodic table was in a cylinder, but couldn’t get it to print that way?

A

Dmitri Mendeleev

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9
Q

Who was able to predict characteristics of undiscovered elements?

A

Dmitri Mendeleev

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10
Q

Who used X-rays to determine the atomic number of elements?

A

Henry Mosely

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11
Q

Who arranged the periodic table based on atomic mass?

A

Henry Mosley

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12
Q

Who developed the compact periodic table by placing the f-block below the d-block?

A

Glenn T. Seaborg

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13
Q

Who arranged the periodic table based on atomic number?

A

Glenn T. Seaborg

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14
Q

Who discovered 100 different isotopes?

A

Glenn T. Seaborg

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15
Q

Who described the idea of a triad–groups of 3 elements that shared similar properties?

A

Johann Dobereiner

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16
Q

What is the conversion of an atom of one element to an atom of another element? Process of changing one element to another through radioactive decay.

A

Transmutation

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17
Q

1-92 occur naturally, but 3 elements not found on Earth; Technetium, Promethium, and Neptunium

A

Natural elements

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18
Q

Elements 1-26 are made from cores of stars, 27-92 made from supernova explosions

A

Where natural elements are made

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19
Q

What is radioactive decay in which an electron is emitted? No change in mass of the particle only a change in the number of protons and neutrons.

A

Beta decay

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20
Q

A nuclear reaction in which an atom emits an alpha particle consisting of 2 protons 2 neutrons. This increases the atomic number by 2 and the mass number by 4.

A

Alpha decay

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21
Q

What is the first type of particle accelerator, invented by Lawrence Ernest, that accelerates charged particles along a spiral path?

A

Cyclotron

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22
Q

What is a horizontal row of elements on the periodic table?

A

Period

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23
Q

The vertical columns in the periodic table. Also called families.

A

Groups

24
Q

When the elements are arranged in increasing atomic numbers, there is a periodic repetition of their physical and chemical properties.

A

Periodic law

25
Q

The electrons in the outermost shell (the main energy level) of an atom; are the electrons involved in forming bonds.

A

Valence electrons

26
Q

A predictable change in a particular direction

A

Trend

27
Q

Distance from the center of the nucleus of an atom to the outermost stable electron orbital in a stable atom

A

Atomic radius

28
Q

Increases down in a group decreases across a period from left to right

A

Atomic radius trend

29
Q

The amount of energy required to remove an electron from an atom.

A

Ionization energy

30
Q

Decreases from top to bottom in a group; increases from left to right in across a period

A

Ionization energy trend

31
Q

The reduction of the attractive force between a positively charged nucleus and its outermost electrons due to the cancellation of some of the positive charge by the negative charges of the inner electrons

A

Electron Shielding

32
Q

The energy change that occurs when an electron is acquired by a neutral atom. the energy change associated with the addition of an electron to a gaseous atom

A

Electron Affinity

33
Q

Increases up and to the right to fluorine. Noble Gasses have lowest

A

Electron affinity trend

34
Q

A measure of the tendency of an atom to attract a bonding pair of electrons. the ability of an atom to attract electrons when the atom is in a compound

A

Electronegativity

35
Q

Decreases from top to bottom in a group; increases from left to right in a period. Except for group 18 which is the lowest

A

Electronegativity trend

36
Q

Elements that are good conductors of electric current and heat, have luster, malleable & ductile, loosely held valence electrons, cations

A

Metals

37
Q

Elements that are poor conductors of heat and electricity, non-lustrous, brittle solids, tightly held valence electrons, anions

A

Nonmetals

38
Q

Group 1, 1 electron in outer hell, M.C.I = +1, very reactive, soft, silver, shiny, low density; Lithium, Sodium, Potassium, Rubidium, Cesium, Francium

A

Alkali Metals

39
Q

Elements that have properties of both metals and nonmetals

A

Metalloids

40
Q

Group 2, 2 electrons in outer shell, M.C.I. = +2, not as reactive as Group 1, greater density than Group 1; Beryllium, Magnesium, Calcium, Strontium, Barium, Radium

A

Alkaline earth metals

41
Q

Elements in Group 8A(Group 18) of the periodic table. Have no charge, 8 valence electrons, and are gases under normal conditions. (Helium, Neon, Argon, Krypton, Xenon, Radon)

A

Noble gases

42
Q

Contains nonmetals, Group 7A(Group 17) 7 valence electrons in it’s outermost energy level, M.C.I.= -1. Very reactive, contain every phase of normal matter in the group. (Fluorine, Chlorine, Bromine, Iodine, Astatine)

A

Halogens

43
Q

Group 6A (Group 16) elements; 6 valence electrons, M.C.I.= -2, important for normal biological functions; high concentrations are toxic and damaging, especially the heavier ones ( Oxygen, Sulfur, Selenium, Tellurium, Polonium)

A

Chalcogen

44
Q

Group 5A (Group 15), 5 valence electrons, M.C.I. = -3, contains nonmetals, metals, and metalloids; (Nitrogen, Phosphorus, Arsenic, Antimony, Bismuth)

A

Pnictogens

45
Q

an element in the s-block or p-block of the periodic table (Groups 1A, 2A, 3A, 4A, 5A, 6A, 7A, 8A)

A

Main group elements

46
Q

The d-block elements are metals with typical metallic properties (1B-8B)(Groups 3-12)

A

Transition elements

47
Q

Groups 1 and 2

A

s-block

48
Q

groups 13-18

A

p-block

49
Q

groups 3-12; transition metals

A

d-block

50
Q

Lanthanides and actinides, the 14 elements in the rows at the bottom of the periodic table in which electrons fill the seven 4f and 5f orbitals

A

f-block

51
Q

Carbon, hydrogen, oxygen, sulfur, phosphorus, and nitrogen

A

Elements found living organisms

52
Q

Most reactive metal

A

Francium

53
Q

Most reactive nonmetal

A

Flourine

54
Q

a nuclear reaction in which atomic nuclei of low atomic number fuse to form a heavier nucleus with the release of energy

A

Nuclear fusion

55
Q

a nuclear reaction in which a heavy nucleus splits spontaneously or on impact with another particle, with the release of energy.

A

Nuclear fission

56
Q

the tendency to recur at regular intervals

A

Periodicity

Freshman Science (1 decks)

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