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Chemistry > Final Semester 1 Review > Flashcards

Final Semester 1 Review Flashcards

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1
Q

The chemical formula in a compound indicates:

a. the source of the elements in the compound.
b. how elements are joined int eh compound.
c. the alchemy symbols for the elements in the compound.
d. the relative proportions of the elements in the compound

A

d.

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2
Q

What happens to matter during a chemical reaction?

A

matter is neither destroyed or created,

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3
Q

The step that usually comes last in solving numeric problems is…

a. calculate
b. measure
c. evaluate
d. analyze

A

c. evaluate

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4
Q

A theory is a…

a. proposed explanation for an observation
b. well-tested explanation for a broad set of observations.
c. summary of the results of many observations
d. procedure used to test a proposed explanation

A

b. a well-tested explanation for a broad set of observations.

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5
Q

An example of an extensive property is…

a. temperature
b. pressure
c. mass
d. hardness

A

c. mass

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6
Q

how to convert from Celsius to Kelvin

A

Kelvin = 273 + x Celsius

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7
Q

How many significant figures in:
0.00350
150050

A

0.00350- 3

150050- 5

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8
Q

What does the number 84 in the name krypton-84 represent?

a. the atomic number
b. the mass number
c. the sum of the protons and electrons
d. twice the number of protons

A

b. the mass number

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9
Q

All atoms of the same element have the same…

a. number of neutrons
b. number of protons
c. mass numbers
d. mass

A

b. number of protons

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10
Q

Which of the following is true about subatomic particles?

a. Electrons are negatively charged and are the heaviest subatomic particle.
b. Protons are positively charged and the lightest subatomic particle.
c. Neutrons have no charge and are the lightest subatomic particles.
d. the mass of a neutron nearly equals the mass of a proton.

A

d. the mass of a neutron nearly equals the mass of a proton.

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11
Q

Which model of the atom is thought to be true today?

a. Protons, electrons, and neutrons are evenly distributed throughout the volume of the atom.
b. The nucleus is made of protons, electrons, and neutrons.
c. Electrons are distributed around the nucleus and occupy almost all the volume of the atom.
d. the nucleus is made of electrons and protons.

A

c. Electrons are distributed around the nucleus and occupy almost all the volume of the atom.

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12
Q

What charge does and electron have?

A

A negative charge.

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13
Q

The nucleus is made up of what?

A

protons and neutrons

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14
Q

What charge does a proton have?

A

positive charge.

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15
Q

What charge does a neutron have?

A

no charge. neutral.

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16
Q

What model did JJ Thomson propose?

A

The Plum Model

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17
Q

How does the energy of an electron change when the electron moves closer to the nucleus?

A

It decreases

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18
Q

When an electron moves from a lower to a higher energy level, the electron…

a. always doubles its energy
b. absorbs a continuously variable amount of energy
c. absorbs a quantum of energy
d. moves closer to the nucleus.

A

c. absorbs a quantum of energy

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19
Q

Emission of light from an atom occurs when an electron…

A

drops from a higher to a lower energy level.

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20
Q

The quantum mechanical model of the atom involves what?

A

the probability of finding an electron in a certain position.

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21
Q

what information does a molecular formula provide?

A

the number and kind of atoms present in a molecule

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22
Q

What is the representative unit of a molecular compound?

A

a molecule

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23
Q

The side-by-side overlap of p orbitals produces what kind of bond?

A

A pi bond

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24
Q

What is the VSEPR theory?

Study These Flashcards
A

repulsive forces between unshared pairs of electrons

25
How does calcium obey the octet rule when reacting to form compounds? a. it gains electrons b. it gives up electrons, c. it foes not change it's number of electrons d. Calcium does not obey the Octet rule.
b. It gives up electrons.
26
What happens in an ionic bond?
oppositely charge ions attract.
27
What does the term coordination number in ionic crystals refer to?
the number of oppositely charged ions surrounding a particular ion.
28
Under what conditions can potassium bromide conduct electricity?
When melted or dissolved in water.
29
What characteristic of metals make them good conductors?
They have mobile valence electrons.
30
An ionic bond is a bond between a...
cation and anion.
31
Why are ionic compounds brittle?
They are brittle because the cations and anions are not free flowing. When hit, the cations come in contact with cations and the like charges repel causing the material to shatter.
32
What type and charge of ion do transition metals form?
Transition metals for Pseudo Noble Gas configurations with a variable charge of 2+.
33
Explain why CaO has a higher melting point than NaCl.
CaO has a higher melting point due to Coulomb's law. It takes more energy to separate CaO than NaCl because in CaO, the oxygen has to gain two electrons as opposed to one.
34
How to determine the protons, electrons, and neutrons.
``` protons are always the same. electrons=protons unless ion neutrons= mass# - atomic# Oxygen Neutrons: 16-8 = 8 ```
35
Why is the second ionization energy always greater than the first ionization energy?
because it is more difficult to remove a second electron from an atom.
36
What is electron shielding?
the effect of inner electrons on the attraction between the nucleus and the outer electrons of an atom.
37
Why does the atomic radius generally increase with atomic number in each group?
the number of energy levels increases.
38
Compare the relative size of an ion to its neutral atom.
the radius of an anion is greater than the radius of its neutral atom.
39
Why does ionization energy decrease as you go down a group?
because as you go down a group, the shielding increases. The shielding decreases the ionization energy.
40
Why does the atomic size decrease across a period?
because the effective nuclear charge increases from left to right in a period.
41
extensive vs. intensive
extensive depend on the extent
42
Describe Democritus' atomic philosophy
-Atoms were indivisible and indestructible | 460-370 bc
43
Describe Dalton's atomic theory
-By using experimental methods, Dalton transformed Democritus's ideas on atoms into a scientific theory. -All elements are composed of atoms -atoms of the same element are identical -atoms of different elements can physically mix or combine in whole number ratios -chemical reactions occur when atoms are separated, joined, or rearranged. 1766-1844
44
Rutherford
-gold foil experiment -in the nuclear atom, the protons and neutrons are located in the positively charged nucleus. -The electrons are distributed around the nucleus and occupy almost all of the volume of the atom. 1911
45
JJ thomson
discovered electron using cathode ray tube | 1897
46
Bohr model
bohr proposed that an electron is found only in specific circular paths, or orbits, around the nucleus.
47
aufbau principle
electrons occupy the lowest energy first
48
pauli exclusion principle
an atomic orbital may describe at most two electrons
49
Hunds rule
electrons occupy orbitals of the same energy in a way that makes the number of electrons with the same spin direction as large as possible.
50
Electromagnetic spectrum from low energy to high energy:
``` radio waves radar microwaves infrared visible ultraviolet xrays gamma ```
51
radio waves have high or low: - energy - frequency - wavelength
radio waves have: - low energy - low frequency - large wavelength
52
relationship of energy frequency and wavelength
low energy, low frequency, big wavelength
53
What is the heisenberg uncertainty principle?
it is impossible to know both the velocity and position of a particle at the same time.
54
How did mendeleev order his periodic elements?
increasing atomic mass
55
what is the periodic law?
when elements are arranged in order of increasing atomic number, there is a periodic repetition of their physical and chemical properties.
56
Where are nonmetals and metalloids?
metalloids are hugging diagonal line | nonmetals are top right corner and hydrogen
57
Types of metals from left to right
``` alkali metals alkaline earth metals transition metals halogen noble gases ```
58
Types of intermolecular force
van de waals forces dipole interactions dispersion forces

Chemistry (6 decks)

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