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Viewing All Flashcards for Science 1-90
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1)
The primary application of chemistry, prior to the Scientific Revolution, was...
 
Metalworking
2)
One of the earliest manufactured alloys was...
 
Bronze
3)
Bronze is an alloy containing a mixture of...
 
Copper and tin
4)
Gunmetal is a type of bronze that contains copper, tin, and...
 
Zinc
5)
Aristotle's five components of nature and matter were...
 
Earth, fire, water, air, and aether
6)
Early scientist studied reactions of metals and carbon compounds heated in the air referred to as...
 
Oxidation
7)
To explain the oxidation processes such as combustion, Lavoisier called a fire-like element as...
 
Phlogiston
8)
The French scientific community reached its peak of excellence during the...
 
18th century
9)
In 1896, Becquerel discovered that uranium was...
 
Radioactive
10)
Approximately how many distinctive elements are known?
 
120
11)
Each element has a specific chemical behavior determined by its...
 
Internal structure
12)
Although atoms are small, by measuring relative mass ratios, chemists have established a table of...
 
Atomic masses
13)
In modern labs, using mass spectrometers, scientists can determine the relative masses of a...
 
Single atom
14)
The symbol format used by chemists, for isotopes, is...
 
A X Z
15)
Atoms with the same number of protons, but differing in neutrons are referred to as...
 
Isotopes
16)
Unstable atoms that decay over a period of time are said to be...
 
Radioactive
17)
The most common usage of carbon-14 isotype is
 
Dating old objects or organisms
18)
When atoms are subjected to heat, the electrons become
 
Excited
19)
A quantum of light energy is also known as a(n)
 
Photon
20)
In Bohr's atomic model, what is located in the center?
 
Protons and neutrons
21)
In Bohr's atomic model, what is located in the periphery?
 
Electrons
22)
The wave particle theory suggests that light is both
 
Wave and particle in behavior
23)
In a modern Quantum mechanical model electrons are considered as a
 
Electron cloud
24)
The number and shape of atom's orbital(s) determines
 
Bonding
25)
On the periodic table, as each element is added, what increases?
 
Protons and atomic number
26)
Period 2 on the Table begins with element
 
3 - Lithium
27)
If added electrons are approximately the same distance from the nucleus, an increased attraction
 
Shrinks the atomic radius
28)
The force of attraction holding an electron to its nucleus is called
 
Ionization energy
29)
The amount of energy change when an element is added to a neutral atom to form a negative ion is called
 
Electron affinity
30)
On the periodic table, the elements in a vertical column are called
 
Group
31)
Outer electrons are shielded from nuclear attractive
 
Pull
32)
On the periodic table, electronegativity
 
Increases across a periodand decreases down a group
33)
The "cluster" of atoms that only break apart when energy is applied are called
 
Chemical compounds
34)
The formula SiO2 is used for a compound named
 
Silica
35)
Attraction that exists between molecules of proximity are referred to as
 
Intermolecular forces
36)
Electron transfer between atoms in attraction between the charged ions is called a(n)
 
Ionic bond
37)
Electron sharing between atoms that results in an attraction that holds the nuclei together is a(n)
 
Covalent bond
38)
A sea of electron clouds that move freely in an element resulting in a strong force of attraction and responsible for electrical conductivity of the metal are called
 
Metallic bonds
39)
What is the energy kJ/mol in ionic bonds?
 
400-4000
40)
What is the energy kJ/mol incovalent bonds?
 
150-1100
41)
What is the energy kJ/mol inmetallic bonds?
 
75-1000
42)
Intermolecular forces resulting from partial changes on molecules are called
 
Van der Waals Force
43)
Bonds that form between a hydrogen and another electronegative atom especially N, O, or F are called a(n)
 
Hydrogen bond
44)
What type of force holds the nitrogen bases together in a DNA molecule, and gives double helical structure for DNA?
 
Hydrogen bond
45)
What important genetic processes are possible because of the hydrogen bonds in DNA?
 
Duplication, replication, transcription, and translation
46)
How are electron molecular orbitals derived?
 
By combining atomic orbitals or hybrid orbitals from each atom of the molecule, or other molecular orbitals from groups of atoms
47)
What is the difference between a sigma and a pi bond?
 
A sigma is the end-to-end overlap of the bonding orbitals, or hybrid orbitals (a single bond), while a pi bond is the side-to-side overlap of unhybridized p-orbital (a pi bond along with a sigma bond form a double bond)(me: this isa freaking long answer)
48)
Briefly describe the resonance concept model.
 
The Resonance Model considers molecules to be an intermediate (called a resonance hybrid) between several Lewis structures that differ only in the placement of the valence electrons.
49)
Numbers assigned to atoms that represent lost or gained electrons are called
 
Oxidation states or oxidation number
50)
A model that helps predicting the geometry of the molecule by focusing on the central atom is called
 
Valence Shell Electron Pair Repulsion (VSEPR) model
51)
Nuclear transformations are acheived by bombarding one type of atom with another atom or with a(n)
 
Alpha particle, or nuetron
52)
What happens in the fission of 235U?
 
When bombarded with the neutrons their nuclei split releasing 2 or 3 more neutrons that then split in the nuclei of other U-235 atoms, releasing more energy and more neutrons. The process continues resulting in an enormous amount of energy (in the form of heat) from a small amount of U. This is called Chain reaction.eww long answer
53)
What happens when fusion of deutrium with tritium occurs?
 
A deutrium nucleus fusing with a tritium nucleus forms an alpha particle (Helium-4 nucleus) an a neutron (17.6 million electron volts(MeV) of released kinetic energy) through the loss of mass in the fusion process.
54)
State the algebraic equation for Boyle's Law.
 
PV = C
55)
State the algebraic equation for Charle's Law.
 
V/T = D
56)
A measurement of temperature that starts at -273°C is
 
0 Kelvin
57)
What equation is derived when you combine Boyle's and Charle's Law?
 
PV/T = CD
58)
State Dalton's Law of partial pressure.
 
The total pressure of a gas mixture equals the sum of the partial pressures of gas components that make up the mixture.
59)
When is Dalton's law useful?
 
To determine partial pressure of a gas component in a gas mixture.
60)
The 1st assumption of the kinetic molecular theory is that identical molecules are
 
Small and occupy negligible volume
61)
The2nd assumption of the kinetic molecular theory is that identical molecules ar
 
Moving quickly, but not at the same speed
62)
The3rd assumption of the kinetic molecular theory is that identical molecules are
 
No force of attraction or repulsion exists
63)
The4th assumption of the kinetic molecular theory is that pressure results from
 
Collisions against a wall
64)
State the equation for Boltzmann's constant.
 
3/2 kTwhere T = temperature in Kelvinand k = Boltzmann constant
65)
State the ideal gas equation.
 
PV = nRT
66)
What happens to He under extreme temperature?
 
Fusion of helium atoms
67)
Outside of a vacuum, gas molecules cannot move in
 
Straight lines
68)
Gases are considered "ideal" when they do not have
 
Intermolecular forces
69)
What type of order exists in gases?
 
None
70)
What type of order exists in a liquid?
 
Loose ordering with random distribution
71)
What type of general ordering exists in a solid?
 
High degree of short-range order
72)
Which state of water is hardly detectable to unaided eye?
 
Vapor
73)
Chemical compounds, or elements, that are able to exhibit different forms of solid forms are called
 
Allotropes
74)
A hexagonal closest-packed metal has ___ neighbors.
 
Twelve
75)
Diamond is formed at
 
High temperature and pressure
76)
A body-centered cubic metal has ___ neighbors.
 
Eight
77)
A cubic closest-packed metal has___ neighbors.
 
Twelve
78)
If a metal is malleable, it can be
 
Beaten into different shapes
79)
If a metal is ductile, it can be
 
Pulled into wire
80)
Closely packed particles within a metal cause it to be
 
Softer
81)
Impurities are added to metals to make them
 
Harder
82)
What kind of equilibrium exists within a system of phase changes?
 
Particles come out and go in at equal rates.
83)
The point of pressure and temperature where a solid, liquid, and gas coexist is called
 
Triple point
84)
The temperature and pressure at which distinction between a gas and a liquid are not obvious is
 
Critical point
85)
Why is it difficult to observe liquid carbon dioxide?
 
CO2 has an atmospheric pressure below the triple point therefore dry ice sublimes directly to vapor in ambient air. It is possible to observe liquid carbon dioxide - in a pressure vessel.
86)
Solutions are mixtures of substances that are
 
Homogenous
87)
In a solution, the larger portion is the
 
Solvent
88)
In a solution, the smaller portion is the
 
Solute
89)
A solution in which the solvent is water is referred to as
 
Aqueous solutions
90)
The amount of solute that can dissolve in a fixed amount of solvent is called
 
Solubility
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