Chapter 2 and 3 QUIZ

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36 Terms

1
What are atoms, according to Dalton's Model?
Indivisible particles that make up all matter.
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2
What does J.J. Thomson's model of the atom propose?
Atoms have negatively charged electrons scattered in a positively charged area, often referred to as the 'plum pudding' model.
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3
What did Ernest Rutherford's model introduce about the atom?
It proposes that there is a small positively charged nucleus at the center of the atom.
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4
Describe the Bohr model of the atom.
It has a positive nucleus with negative electrons surrounding it, and the attraction between these particles prevents electrons from leaving.
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5
What happens to an electron when an atom absorbs energy?
The electron moves to a higher energy level (excited state), which is unstable, and it eventually falls back to the ground state, emitting energy in the form of EM radiation.
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6
What is quantization in the context of atomic energy?
The concept that energy levels of an atom are limited to certain fixed values, rather than being continuous.
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7
What defines isotopes?
Atoms that have the same number of protons but different numbers of neutrons.
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8
What is the purpose of a mass spectrometer?
To measure the masses of different isotopes and their relative abundances.
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9
Explain the trend in ionization energy across a period.
Ionization energy increases across a period due to increasing nuclear charge, which enhances the attraction between the nucleus and outer electrons.
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10
What is the significance of effective nuclear charge?
The actual charge experienced by valence electrons, accounting for shielding effects from inner electrons.
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11
How do atomic radii change across a period and down a group?
Atomic radius decreases across a period and increases down a group.
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12
What is the relationship between electronegativity and atomic structure?
Electronegativity increases across a period and decreases down a group; higher nuclear charge leads to stronger attraction for bonding electrons.
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13
What is unique about the coordination number in complexes?
The number of dative covalent bonds formed between the ligand and the central metal ion.
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14
What does Heisenberg's Uncertainty Principle state?
It is impossible to know both the exact position and momentum of an electron simultaneously.
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15
What is the Aufbau Principle?
Electrons are filled into the lowest energy orbitals first before moving to higher energy levels.
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16
What is the role of the ligand in transition metal complexes?
Ligands donate a lone pair of electrons to form dative covalent bonds with the central metal ion.
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17
Describe how transition metal complexes absorb light.
They absorb visible light due to partially filled d orbitals, which are split into two energy sublevels by the electric field of the ligands.
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18
What is a resonance structure?
A set of two or more Lewis structures that represent the same molecule, indicating the distribution of electrons.
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19

What does electronegativity indicate?

The tendency of an atom to attract electrons towards itself in a chemical bond.

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20

Explain hybridization in chemistry.

The process of combining atomic orbitals to create new hybrid orbitals for bonding.

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21

What are transition metals?

Elements that have partially filled d orbitals and exhibit variable oxidation states.

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22

What is a ligand in coordination chemistry?

A molecule or ion that donates a pair of electrons to a central metal ion in a complex.

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23

What are the key features of metals?

Metals are typically malleable, ductile, conductive, and have a lustrous appearance.

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24

What is the significance of the periodic table's organization?

It reflects the periodic trends in element properties such as atomic size, electronegativity, and ionization energy.

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25

What is the Pauli Exclusion Principle?

No two electrons in an atom can have the same set of quantum numbers, meaning each electron has a unique state.

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26

Explain the difference between endothermic and exothermic reactions.

Endothermic reactions absorb heat, while exothermic reactions release heat.

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27

What is a titration?

A technique used to determine the concentration of a solute in a solution by reacting it with a solution of known concentration.

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28

Define a redox reaction.

A reaction involving the transfer of electrons between two species, leading to changes in oxidation states.

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29

What is a quantum number?

A number that describes the properties of atomic orbitals and the electrons in those orbitals.

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30

What is the concept of oxidation states?

The charge of an atom in a compound, indicating its ability to donate or accept electrons during a chemical reaction.

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31

What characterizes a polar molecule?

A molecule with an uneven distribution of charge, resulting in partial positive and negative poles.

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32

What is enthalpy?

The total heat content of a system, used in thermodynamics to describe energy changes.

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33

Define a ligand in coordination chemistry.

A molecule or ion that donates a pair of electrons to a central metal ion to form a coordination complex.

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34

What is an ionic compound?

A compound formed from the electrostatic attraction between positively and negatively charged ions.

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35

What are the five steps of a mass spectrometer?

  1. Ionization - atoms are ionized to form charged particles. 2. Acceleration - ions are accelerated by an electric field. 3. Deflection - ions are deflected in a magnetic field based on their mass-to-charge ratio. 4. Detection - ions are detected, usually by a mass detector. 5. Data analysis - results are analyzed to determine the masses and abundances of isotopes.

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36

What is oxidation?

Oxidation is the loss of electrons by an atom or ion during a chemical reaction.

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