Atomic Theory

Question 1

Who is accredited with thinking up the law of conservation of mass?

Answer 1

Antoine Lavoisier

Question 2

This law says that “different pure samples of the same compound always contain the same proportions of each element of mass”

Answer 2

The law of definite proportions

Question 3

What were John Dalton’s four postulates?

Answer 3

1) Each element is composed of tiny particles called atoms
2) All atoms of a given element are identical and all atoms of different elements are different
3) Atoms are not created or destroyed in chemical reactions. They are dissociated, combined, or recombined
4) Compounds are formed when atoms of different elements combine with one another. A given compound always contains the same relative numbers and types of atoms

Question 4

Who discovered electrons?

Answer 4

J.J Thompson

Question 5

Who discovered a nucleus with protons in atoms?

Answer 5

Earnest B Rutherford

Question 6

equal to the number of protons plus the number of neutrons

Answer 6

Mass number

Question 7

The number of protons (or electrons in a neutral atom)

Answer 7

Atomic number

Question 8

Same element with a different number of neutrons

Answer 8

Isotope

Question 9

Isotopes of an element exhibit _________ chemical behavior

Answer 9

Identical

Question 10

Atomic mass given in the periodic table is an _________ of all of the isotopes of that element

Answer 10

Average

Question 11

In mass spectrometry, less deflection means a ___________ mass

Answer 11

Larger

Question 12

What is the equation for average atomic mass?

Answer 12

(Mass# x %)+(Mass# x %) = average mass

Question 13

What is the equation for mass percent of an element in a substance?

Answer 13

Mass % of element= (# of atoms of element)(elements atomic mass) / (formula weight of compound) x 100

Question 14

Linear distance covered before a wave starts to repeat itself

Answer 14

Wavelength

Question 15

A low frequency wave has a __________ wavelength

Answer 15

Higher

Question 16

What is the formula for wavelength in its relation to frequency?

Answer 16

C=(wavelength)(v)

Question 17

What is the constant in the formula?

Answer 17

3 x 10^8 m/s

Question 18

Who hypotheses that the energy radiated from a heated objects is emitted in discrete units or quants

Answer 18

Max Planck

Question 19

Plancks constant is represented as ____

Answer 19

H

Question 20

The higher the frequency the _________ the energy

Answer 20

Higher

Question 21

Highly intense _____________ light does not eject any electrons

Answer 21

Low frequency

Question 22

When the __________________ is reached electrons are ejected immediately

Answer 22

Threshold frequency

Question 23

Increasing the intensity of the light at a frequency that will cause electrons to eject results in a ____________ however all electrons share the same velocity

Answer 23

Higher ejection rate

Question 24

Increasing the frequency of the light increases the velocity of the ejected electrons, however all ejected electrons ___________________

Answer 24

Share the same velocity

Question 25

A beam of light is a stream if particles called _________

Answer 25

Photons

Question 26

What is Plancks equation?

Answer 26

E=hv

Question 27

State Coulomb's law

Answer 27

The force of attraction decreases as the distance between the outermost electron and the protons increase

Question 28

The electrons that are furthest from the nucleus are partly _________ by the inner core electrons

Answer 28

Shielded

Question 29

The minimum amount of energy that is required to remove the outermost electron form an atom in its gas phase

Answer 29

First ionization energy

Question 30

Ionization energy generally __________ as you move across the periodic table

Answer 30

Increases

Question 31

Electrons contained in the inner shell

Answer 31

Inner core electrons

Question 32

Electrons contained in the outer shell

Answer 32

Valence electrons

Question 33

N=1 can hold how many subshells?

Answer 33

1

Question 34

What is the subshell n=1 can hold?

Answer 34

1s

Question 35

What subshells does n=2 contain?

Answer 35

2s and 2p

Question 36

How many electrons can subshell 2s hold?

Answer 36

2

Question 37

How many electrons can subshell 2p hold?

Answer 37

6

Question 38

How many electrons can 3s hold?

Answer 38

2

Question 39

How many electrons can 3p hold?

Answer 39

6

Question 40

How many electrons can subshell 3d hold?

Answer 40

10

Question 41

The shielding effect ___________ for each subshell that is added

Answer 41

Increases

Question 42

Electrons furthest from the nucleus have _________ potential energy

Answer 42

Higher

Question 43

According to the QM model, all electrons under the same subshell have __________ energy

Answer 43

The same

Question 44

A graphic representation of the space that and electron will occupy 90% of the time

Answer 44

Orbital

Question 45

Electrons are added to the _______ energy orbitals available

Answer 45

Lowest

Question 46

Atoms with unpaired electrons

Answer 46

Paramagnetic

Question 47

atoms with no unpaired electrons

Answer 47

Diamagnetic atoms

Question 48

The effective nuclear charge (the charge experience by an electron) is written as _______

Answer 48

Zeff

Question 49

As you go across the periodic table the atomic radius __________

Answer 49

Decreases

Question 50

Metals lose elections to form ________

Answer 50

Cations

Question 51

Non-metals fain electrons to form _________

Answer 51

Anions

Question 52

___________ share the same electronic configurations but have different radii

Answer 52

Isolectronic species

Question 53

_________ are smaller than smaller than neutral atoms

Answer 53

Cations

Question 54

________ are larger than neutral atoms

Answer 54

Anions

Question 55

It's harder to pull electrons from a ________ subshell

Answer 55

Full

Question 56

First ionization energy generally _________ as atomic radii decrease

Answer 56

Increase

Question 57

The second ionization potential for an atoms is always __________

Answer 57

Greater

Question 58

An elements ability to attract electrons in a chemical bond

Answer 58

Electronegativity

Question 59

Electrons will spend _______ time around the more electronegative element in a chemical bond

Answer 59

More

Question 60

Electronegativity generally __________ as you move across the periodic table

Answer 60

Increases

Question 61

Electronegativity ________ as atomic radius decreases

Answer 61

Increases

Question 62

Who was the first to think about atomic theory?

Answer 62

Democritus