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Chemistry 10th Grade > STUDY ME > Flashcards

STUDY ME Flashcards

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1
Q

Mole as a number

A

6.02x10^23

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2
Q

How came up with the mole number

A

Avagadro

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3
Q

Heisenbergs contribution to atomic theory

A

The idea that you can not know both an electron’s velocity and it’s location at the same instant.

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4
Q

Rutherford’s contribution to atomic theory

A

Discovered the Nucleus

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5
Q

Thomson’s contribution to atomic theory

A

Discovered electrons

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6
Q

Planck’s contribution to atomic theory

A

The idea that electrons exhibit the behavior of waves and particles

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7
Q

Dalton’s contribution to atomic theory

A

Had evidence in the form of 3 laws that atoms existed

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8
Q

Chadwick’s contribution to atomic theory

A

Isolated a beam of high penetrating power that could go through a film canister and expose photographic plates

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9
Q

Bohr’s contribution to atomic theory

A

He said that electrons must reside in “finite” energy levels

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10
Q

Democritus’s contribution to atomic theory

A

First used the term “atom” with means “indivisible”

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11
Q

DeBroglie’s contribution to atomic theory

A

Gave mathematical relationships between energy and electrons

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12
Q

What evidence did Bohr have to explain the location of electrons in energy levels around the nucleus of a hydrogen atom?

A

specific colors of light (photon of light)

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13
Q

What “uncertainty” did Heisenberg explain in his uncertainty principle?

A

Cannot know both position and velocity of an electron

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14
Q

How did Heisenberg’s uncertainty principle change Bohr’s model

A

probability and orbitals

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15
Q

Who’s model is this?

A

Dalton: Solid Sphere no parts

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16
Q

Who’s model is this?

A

Thomson - Plum pudding

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17
Q

Who’s model is this?

A

Rutherford: Nuclear model

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18
Q

Who’s model is this?

A

Bohr: Move in spherical orbits

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19
Q

Name this region of the periodic table

A

Alkali metals

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20
Q

Name this region of the periodic table

A

Alkaline earth metals

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21
Q

Name this region of the periodic table

A

Transition metals

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22
Q

Name this region of the periodic table

A

Lanthanides (Rare earth metals)

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23
Q

Name this region of the periodic table

A

Actinides

24
Q

Name this region of the periodic table

A

Halogens

25
Q

Name this region of the periodic table

A

Noble gases

26
Q

What is the definition of nuclear charge

A

The nuclear charge is the total charge of all the protons in the nucleus. It has the same value as the atomic number. The nuclear charge increases you go across the periodic table.

27
Q

Define shielding effect

A

The shielding effect is when the electron and the nucleus in an atom have a decrease in attraction which changes the nuclear charge.

28
Q

What is an example of the shielding effect?

A

An example of shielding effect is in nuclear fission when electrons furthest from the center of the atom are pulled away.

29
Q

Define atomic radius

A

the total distance from an atom’s nucleus to the outermost orbital of electron.

30
Q

Define Ionization energy

A

Ionization energy is the energy required to remove an electron from a gaseous atom or ion

31
Q

Define electronegativity

A

Electronegativity is a measure of how strongly atoms attract bonding electrons to themselves. Its symbol is the Greek letter chi: χ.

32
Q

What is this trend for on the periodic table?

A

Shielding Effect

33
Q

What is this trend for on the periodic table?

A

Nuclear Charge

34
Q

What is this trend for on the periodic table?

A

Ionization Energy or Electronegativity

35
Q

What is this trend for on the periodic table?

A

Electronegativity or Ionization Energy

36
Q

What is this trend for on the periodic table?

A

Atomic Radius

37
Q

Why does flurine have a higher ionization energy than iodine?

A

Smaller holds it’s electrons tighter. takes more energy to remove the electron

38
Q

From left to right across the periodic table the atomic radius will _______

A

Decrease

39
Q

From left to right across the periodic table the ionization energy will _______

A

increase

40
Q

From left to right across the periodic table the electronegativity will _______

A

increase

41
Q

what causes the trend in atomic radio to increase down a group on the periodic table

A

addition of energy levels

42
Q

Describe group 2 (alkaline earth metals) as they are considered in order from top to bottom

A

The number of principal energy levels INCREASE and the number of valence electrons REMAIN THE SAME

43
Q

Define ground state

A

is an atom in which the total energy of the electrons can not be lowered by transferring one or more electrons to different orbitals. That is, in a ground-state atom, all electrons are in the lowest possible energy levels

44
Q

Calcium and strontium have similar chemical properties because they both have the same

A

number of valence electrons

45
Q

On the periodic table of the elements all the elements within group 16 (the oxygen family or chalcogens) have the same number of?

A

valence electrons

46
Q

An element with a partially filled “d” sublevel in the ground state is classified as

A

a transitional metal

47
Q

as each successive element in group 15 (Nitrogen family) is considered in order of increating atomic number, the atomic radius

A

Increases

48
Q

The strength of an atmos attration for the electrons in a chemical bond is the atom’s

A

electronegativity

49
Q

Which properties are most common in nonmetals?

A

HIGH ionization energy and HIGH electronegativity

50
Q

As the elements of group 1 (hydrogen and the alkali metals) are considered in order of increasing atomic radius, the ionization energy of each successive element generally

A

Decreases

51
Q

The amount of energy required to remove the outermost electron from a gaseous atom in the groud state is known as

A

ionization energy

52
Q

Why does the ionization energy of each succesive element in group 1 decrease?

A

increasing radius and increasing shielding effect

53
Q

Compared to the atomic radius of a sodium atom the atomic radius of a magnesium atom is smaller. The smaller radius is primarily a result of the magnesium atom having

A

a larger nuclear charge

54
Q

What element has the LEAST attraction for electrons in a chemical bond?

Oxygen, flurine, nitrogen, orchlorine

A

Nitrogen

55
Q

The ability of carbon to attract electrons is

A

less than that of nitrogen and oxygen

56
Q
A

Chemistry 10th Grade (4 decks)

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