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Introduction To Chemistry > The Structure of The Atom & The Periodic Table > Flashcards

The Structure of The Atom & The Periodic Table Flashcards

Learn about the structure of atoms & understanding the Periodic Table

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1
Q

What is the basic structural unit of an element?

A

Atom

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2
Q

What is the smallest unit of an element that retains the chemical properties of the element?

A

Atom

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3
Q

Atoms consist of three primary particles. Name them.

A

Protons, neutrons, & electrons.

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4
Q

What is a the name of the small, dense positively charged region in the center of the atom?

A

Nucleus

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5
Q

The nucleus, small, dense, positively charged region in the center of the atom contains:

A
  • Protrons (positively charged particles)

- Nuetrons (uncharged particles)

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6
Q

What is the name of the negatively charged particles located outside of the nucleus of an atom?

A

Electrons

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7
Q

These move very rapidly in a relatively large volume of space while the nucleus is small and dense.

A

Electrons

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8
Q

Protons and electrons have charges that are equal in magnitude but….

A

Opposite in sign

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9
Q

A ________ atom (no electrical charge) has the same number of protons and electrons.

A

Neutral

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10
Q

What does the atomic number represent?

A

The number of protons in the atom.

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11
Q

What does the mass number represent?

A

The sum of the number of protons and neutrons.

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12
Q

True or false: The mass number usually listed to the left (upper left) of the symbol of the atom and above the atomic number?

A

True

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13
Q

Number of protons + number of neutrons=

A

Mass number

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14
Q

Mass number - number of protons=

A

Number of neutrons

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15
Q

Mass number - atomic number =

A

Number of neutrons

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16
Q

__________: atoms of the same element having different masses.

A

Isotopes

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17
Q

What contains the SAME number of protons but DIFFERENT numbers of neutrons?

A

Isotopes

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18
Q

Protons are the _________ number.

A

Atomic

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19
Q

If you change protons, what changes?

A

The element.

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20
Q

Isotopes of the same element have ___________ chemical properties.

A

Identical

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21
Q

True or false: Some isotopes ARE radioactive.

A

True

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22
Q

What does the number, 35.45, under Chlorine represent? (This number is located under the symbol of the element.)

A

It is the atomic mass. This is NOT the mass number of an isotope.

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23
Q

True or false: The number under an element symbol is the mass number of an isotope.

A

False

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24
Q

__________ ___________ is an average corrected by the relative amounts of each isotope present in nature.

A

Weighted average

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25
Q

Determining atomic mass:

  • Convert % to a decimal fraction(divide % by 100).
  • Multiply the decimal fraction by the mass of that isotope to determine the contribution of each isotope.
  • Add the mass contributed by each isotope.
  • Don’t forget the units (amu)!!!
A

*Don’t forget the units (amu)!!!

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26
Q

True or false:
Atomic mass determination.
Abundance ÷100 × mass(amu)= atomic mass
-then add all sums of each naturally occurring isotope.

A

True. You must round to significant figures BEFORE adding all of the sums together.

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27
Q

________ ________ ________ : the first experimentally based theory of atomic structure.

A

Dalton’s Atomic Theory

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28
Q

6 Postulates of Dalton’s Atomic Theory

A
  1. All matter consists of tiny particles.
  2. An aton cannot be created, divided, destroyed, or converted to any other type of atom.
  3. Atoms of a particular element have identical properties.
  4. Atoms of different elements have different properties.
  5. Atoms of different elements combine in simple whole-number ratios to produce compounds (stable combinations of atoms)
  6. Chemical change involves joining, separating, or rearranging atoms.

Postulates 1, 4, 5 & 6 are still regarded as true.

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29
Q

_________ were the first subatomic particles to be discovered using the cathode ray tube.

A

Electrons

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30
Q

True or false: Protons were discovered by Goldstein.

A

True. Protons are the same size charge but opposite in sign & is 1837 times heavier than an electron.

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31
Q

Neutrons = ______ charge

A

Zero

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32
Q

________ are 1837 times heavier than an electron.

A

Protons

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33
Q

_________ are almost the same mass as the proton.

A

Neutrons

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34
Q

Rutherford’s “____ ____ __________” lead to the understanding of the nucleus.

A

Gold Foil Experiment

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35
Q

Rutherford’s Gold Foil Experiment

A
  • most of the atom is empty space.

- the majority of the mass is located in a small, dense region

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36
Q

What is the study of information obtained from absorption or emission of light by atoms?

A

Spectroscopy. It is used to understand the electronic structure.

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37
Q

To understand the electronic structure, we must first understand light, which is the ……

A

Electromagnetic Radiation

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38
Q

Electronic Radiation

  • travels in waves from a source
  • speed of 3.0 × 10^8 m/s
A

True

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39
Q

Distance between 2 waves = _____________

A

Wavelength

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40
Q

The height of a wave = _____________

A

Amplitude

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41
Q

True or false: Each wavelength travels at the same velocity, but has its own characteristic energy.

A

True

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42
Q

____________ is the distance between identical points on successive waves.

A

Wavelength

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43
Q

Electromagnetic Spectrum
High energy = short wavelength [into 10^(-)]
Low energy = long wavelength [into 10^(+)]

A

True

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44
Q

The Bohr Atom

  • atoms can absorb & enit energy via promotion of electrons to higher energy levels & relaxation to lower levels.
  • energy that is emitted upon relaxation is observed as a single wavelength of light.
  • spectral lines are a result of electron transitions between allowed levels in the atoms.
A

True.

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45
Q

Model of The Bohr Atom:

Electrons exist in fixed energy levels surrounding the nucleus. This is….

A

Quantization of energy

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46
Q

Model of The Bohr Atom:

Promotion of electron occurs as it absorbs energy is……

A

The Excited State

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47
Q

Model of The Bohr Atom:

Energy is released as the electron travels back to lower levels is……

A

Relaxation

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48
Q

The amount of energy absorbed in jumping from one energy level to a higher energy level is a _________ _________.

A

Precise quantity

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49
Q

__________ what Bohr called the fixed energy level.

A

Orbit

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50
Q

What is the lowest possible energy state?

A

Ground state

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51
Q

True or false: In the Bohr Theory, electrons are found only in allowed energy levels.

A

True

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52
Q

Modern Atomic Theory:

  • Bohr’s model of the atom failed to explain line of spectra of atoms with more than one electron.
  • One MAJOR change from Bohr’s model is that electrons do NOT move in orbits.
  • Atomic Orbitals- regionsin spacewith a high probability of finding an electron.
  • Electrons move rapidly withinthe orbital giving a high energy density.
A

Modern Atomic Theory

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53
Q

________ _________- regions in space with a high probability of finding an electron.

A

Atomic orbitals

54
Q

The physical and chemical properties of the elements are periodic functions of their atomic numbers is called ___________ _____

A

Periodic Law

55
Q

Dmitri Mendeleev and Lothar Meyer- independently developed the precursor to our modern Periodic Table.

A

They noticed that as you list elements in order of atomic mass, there is a distinct regular variation of their properties.

56
Q

Rows on a The Periodic Table are called ________

A

Periods (energy levels)

57
Q

The columns on The Periodic Table are called _________

A

Groups

58
Q

The far left column (Group 1) on the Periodic Table are ___________ metals.

A

Alkali

59
Q

The second column (Group 2) are ____________ metals.

A

Alkaline

60
Q

Groups 3- group 12 on the Periodic Table are _____________ metals.

A

Transition

61
Q

Group 17 on the Periodic Table are ____________.

A

Halogens

62
Q

Group 18 on the Periodic Table are ________ ________.

A

Noble gases

63
Q

On the Periodic Table, atomic numbers 58- 71 are ____________.

A

Lanthanidee

64
Q

On the Periodic Table, atomic numbers 90-103 are _____________.

A

Actinidee

65
Q

True or false: Inner transition elements or rare earth elements are ( zoomed in from energy levels 6 &7 so you can see) located at the bottom of the Periodic Table.

A

True

66
Q

Columns on the Periodic Table are called groups or also called ________.

A

Families

67
Q

Classification of Elements:

__________- elements that tend to lose electrons during chemical change, forming positive ions.

A

Metals

68
Q

Classification of Elements:

____________ - elements that tend to gain electrons during chemical change, forming negative ions.

A

Non-metals.

69
Q

What are poor conductors of electricity?

A

Non-metals. They are dull/not shiny and will not shape.

70
Q

What are high conductors of electricity?

A

Metals. They are shiny and malleable (hammered or pressed. You can beat into a shape)

71
Q

____________ - have properties intermediate between metals and nonmetals.

A

Metalloids

72
Q

True or false: ALL elements touching the zig zag line on the Periodic Table are metalloids.

A

False. All elements touching the zig zag line on the Periodic Table are metalloids EXCEPT for aluminum.

73
Q

__________ _____________- describes the arrangement of electrons in atoms.

A

Electron configuration

74
Q

__________ ___________- are the outermost electrons

A

Valence electrons

75
Q

The Quantum Mechanical Atom:

Schröedinger developed equations that took into account the particle nature and the wave nature of the electrons.

A

True

76
Q

Schröedinger’s equations

Equations that determine the probability of finding an electron in a specific region in space, quantum mechanics.

A
  • principle energy levels ( n= 1,2,3…)
  • each evergy level has 1 or more sublevels or subshells (s,p,d,f)
  • each sublevel contains 1 or more atomic orbitals
77
Q

Energy Levels and Sublevels

True or false: The larger the value of n, the higher energy level and the farther away from the nucleus the electrons are.

A

True.

78
Q

True or false: The number of sublevels in a principal energy level is equal to n.

A

True.

  • in n=1, there is one sublevel
  • in n=2, there are two sublevels
79
Q

Principal Energy Levels

The electron capacity of a principal energy level (or total electrons it can hold) is 2(n)^2

A

True.

  • n=1 can hold 2(1)^2= 2 electrons
  • n=2 can hold 2(2)^2= 8 electrons
80
Q

Principal Energy Levels

How many electrons can be in the n=3 level?

A

2(3)^2=18

81
Q

_________ - a set of energy-equal orbitals within a principal energy level.

A

Sublevel

82
Q

Subshells increase in energy. What are they?

A

s<p></p>

83
Q

True or false: True.

Subshell. Orbitals.

s. 1
p. 3
d. 5
f. 7

A

True.

84
Q

Electron Configuration

What is the Aufbau Principle?

A

You can’t get to 2s until you get 1s. Remember s<p></p>

85
Q

From Geiger’s experiments, Rutherford concluded that the atom contains a small, extremely dense region in which most of the atom’s ________ is concentrated. He called this central region the ___________ of the atom.

A

mass, nucleus

86
Q

Radioactive isotopes have unique ____________ behavior but identical ___________ behavior to their nonradioactive counterparts, which allows them to serve as monitoring agents for biochemical systems.

A

nuclear, chemical

87
Q

True or false:

Atoms combine randomly to form compounds.

A

False. Atoms always combine in the same ratio to form a given compound.

88
Q

True or false:

According to Dalton’s Theory, chemical change involves separating, joining, or rearranging atoms.

A

True.

89
Q

Light is also referred to as electromagnetic radiation and travels in the form of _________, but also has properties characteristic of ____________.

A

Waves, particles

90
Q

Radiation from a particular point on the electromagnetic spectrum has a unique _____________, but all electromagnetic radiation travels the speed of light.

A

Wavelength

91
Q

What is a wavelength?

A

The distance between identical points on two successive waves.

92
Q

True or false:

Atoms in the gas phase only emit radiation at specific wavelengths.

A

True. Each atom has a unique emission spectrum with radiation at specific wavelengths.

93
Q

Energy can only have certain values and cannot have amounts between those values. This is referred to as the _____________ of energy.

A

Quantization

94
Q

A spectral line in the emission spectrum of an atom represents …….

A

A photon of light being emitted when an electron moves from a higher energy state to the ground state of an atom.

95
Q

True or false:

An atomic orbital represents the probability of finding an electron in a region of space.

A

True.

96
Q

A __________ is a substance whose atoms tend to lose electrons during chemical change.

A

Metal. On the other hand, a nonmetal is a substance whose atoms may gain electrons.

97
Q

The modern ____________ law states that the physical and chemical properties of the elements display a certain periodicity related to their atomic ____________.

A

Periodic, numbers.

98
Q

True or false:

Elements in the same group of the periodic table have similar chemical properties.

A

True.

99
Q

True or false:
The modern periodic law states that the physical and chemical properties of elements are periodic functions of their atomic numbers.

A

True.

100
Q

All elements in Groups 1A to 8A of the periodic table are called the ________________ metals.

A

Main-group

101
Q

Elements in the B groups are called the _____________ metals.

A

Transition

102
Q

An _________ __________ is a specific region of a sublevel containing a maximum of two electrons.

A

Atomic orbital

103
Q

What is the relationship that correctly describes the maximum number of electrons that each principal energy level can hold?

A

2(n)^2

104
Q

A set of equal-energy orbitals within a principal energy level is called a ____________.

A

Sublevel.

105
Q

An atomic ___________ is a specific region of space within a sublevel that can contain a maximum of ___________ electrons.

A

Orbital, two.

106
Q

What requirement must be met for two electrons to coexist in the same orbital?

A

The electrons must have opposite spins.

107
Q

Two electrons in one orbital that possess opposite spins are referred to as __________ electrons.

A

Paired.

The number and arrangement of unpaired electrons in an atom are responsible for the magnetic properties of elements.

108
Q

Aufbau Principle:

A

Electrons fill the lowest energy orbitals first.

109
Q

Pauli’s Exclusion principle:

A

Each orbital can hold up to two electrons with spins paired.

110
Q

Hund’s Rule:

A

When there is a set of equal-energy orbitals, each orbital becomes half-filled before any become completely filled.

111
Q

Why are s,p,d, and f blocks designated as such?

A

The block designation indicates the subshell that is being filled with electrons.

112
Q

In order to write the electron configuration of an atom, the number of _____________ must be known, and this number is equal to the atomic ____________ for a neutral atom.

A

Electrons, number.

113
Q

Notation & meaning.

1s^2

1=
S=
2=

A 
1= principal of energy 
S= sublevel
2= number of electrons in a sublevel
114
Q

The octet rule states that elements will react by gaining, losing, sharing electrons in order to attain the same electron configuration as their closest _____________ gas.

A

Noble

115
Q

What are valence electrons?

A

The outermost electrons in an atom.

116
Q

An ion with more electrons than its neutral atom is called a(n)

A

Anion

117
Q

An ion with fewer electrons than its neutral atom is called a(n)

A

Cation

118
Q

The charge of an ion with more electrons than its neutral atom is

A

Negative

119
Q

The charge of an ion with fewer electrons than its neutral atom is

A

Positive

120
Q

When forming an ion, a metal will ________ electrons and a nonmetal will _________ electrons in order to attain the same electron configuration as the closest noble gas.

A

Lose, gain.

121
Q

True or false:

Ions are formed by gain or loss of electrons.

A

True.

122
Q

Recall the total electron capacities of the orbital types:

A

S: holds two electrons
P: holds six electrons
D: holds ten electrons
F: holds 14 electrons

123
Q

Both transition metals and representative metals ___________ electrons when forming ions. However, transition metals differ from representative metals by forming ions of _____________ type(s) of charge(s).

A

Lose, multiple.

124
Q

Facts:

  • Positive ions (cations) are smaller than their parent atoms.
  • The cation has more protons than electrons.
  • The decrease in the number of electrons pulls the remaining electrons closer to the nucleus.
  • Also, cation formation often results in the llss of all outer-shell electrons, resulting in a significant decrease in radius.
A

All true.

125
Q

Facts:

  • Negative ions (anions) are larger than their parent atoms.
  • The anion has more electrons than protons.
  • Owing to the excess negative charge, the nuclear “pull” on each individual electron is reduced.
  • The electrons are held less tightly, resulting in a larger anion radius in contrast to the neutral atom.
A

All true.

126
Q

Why does atomic size decrease from left to right across a row of the periodic table?

A

The number of protons in the nucleus increases, pulling the valence electrons closer.

127
Q

True or false:

Ionization energy increases from left to right as the number of protons in the nucleus increases.

A

True.

128
Q

As atomic size decreases, ionization energy ______________,since ‘the electrons are _____________ the protons in the nucleus.

A

Increases; closer to

129
Q

Electron affinity measures the tendency of an element to form a(n) ______________.

A

Anion.

-Electron affinity measures the energy change associates with adding an electron to a neutral atom; i.e., forming an anion.

130
Q

Facts:

  • Electron affinities generally increase across a period.
  • Novle gases have very low values for electron affinity. (Noble gases are very stable and do not readily form anions.)
A

True.

131
Q

In the Bohr model of an atom, electrons only occupy certain allowed ___________ levels, or orbits. Atoms absorb or emit ___________ of light when electrons move between these levels.

A

Energy, photons.

132
Q

Facts:

  • Cathode rays consist of negatively charged particles.
  • Cathode rays are identical no matter their source.
A

True.

Introduction To Chemistry (3 decks)

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