IBC FINAL Flashcards
(96 cards)
1
Q
Know how to calculate average atomic mass for an element based on the data from stable isotopes (percent abundance)
A
each isotope’s mass is multiplied by its abundance and then summed
2
Q
What is the nucleus?
A
- The nucleus is a small, dense region at the center of the atom.
- It consists of positive protons and neutral neutrons,
- Because the protons are positive and neutrons are neutral, it has an overall positive charge
- The nucleus is just a tiny part of the atom, but it contains virtually all of the atom’s mass.
3
Q
What is atomic number?
A
tells how many protons the atom of the element contains, the number of protons in the nucleus of an atom of an element. The atomic number identifies the element.
4
Q
What is mass number?
A
the total number of protons and neutrons in an atom. to find, round atomic mass to nearest whole number.
OR
(the atomic mass rounded to a whole number)
the total number of protons and neutrons in an atom’s nucleus
5
Q
What is an isotope?
A
- atoms of the same element that have different numbers of neutrons
- Atoms of the same element with different mass numbers.
- Same atomic number (same number of protons)
- Different number of neutrons
- Chemically alike
- Every element has naturally occurring isotopes
- Isotopes occur in different abundance levels
- Not all isotopes are stable
6
Q
What is the electron cloud?
A
“massless” electrons circle nucleus billions of times per second
- The location of the electrons in the quantum mechanical model of the atom
7
Q
What is the current atomic theory?
A
the electron cloud model
8
Q
What was Dalton’s atomic theory?
A
mater is made of atoms, and atoms of the same element are identical
9
Q
What was Thomson’s atomic theory?
A
atoms contain subatomic particles
10
Q
what was Rutherford’s atomic theory?
A
atoms have a nucleus surrounded by empty space
11
Q
What was Bohr’s atomic theory?
A
electrons move around the nucleus in circular orbits
12
Q
what was the Shrodinger/Heisenberg atomic theory?
A
electrons move in waves, and an electron cloud surrounding the nucleus represents where an electron should be (also called the electron cloud model)
13
Q
aufbau principle
A
states that each electron occupies the
lowest energy orbital available
14
Q
FREEEE CARDDDDD
A
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15
Q
What 3 subatomic particles do atoms contain?
A
protons, neutrons, and electrons
16
Q
where can you find protons and what is their charge?
A
in the nucleus, positive charge
17
Q
where can you find electrons and what is their charge
A
outside the nucleus, negative charge
18
Q
where can you find neutrons, and what is their charge?
A
in the nucleus, neutral charge
19
Q
what is average atomic mass?
A
the average mass of all isotopes and their abundance
20
Q
What are the 4 orbital shapes?
A
s - sphere, p - peanut, d - double peanut, f - flower
21
Q
what are the steps for electron configuration?
A
- write the number of the energy level (shell)
- write the letter of the orbitals(sublevel or subshell)
- write the number of electrons in that orbital
22
Q
What is the order of the electromagnetic spectrum?
A
radio waves, microwaves, infrared, visible light, ultraviolet, x-rays, gamma ray (raging marshians invaded Venus using x-ray guns)
23
Q
What is wavelength?
A
the distance between crests
24
Q
what is amplitude
A
height from zero to crest
25
What is frequency?
number of wave cycles per unit of time, measured in Hertz (Hz)
26
what is the product of frequency and wavelength?
the speed of light
27
what is the equation for finding wavelength, given frequency?
wavelength = speed of light/frequency
28
how do you find the energy of photons?
E = hv OR E = h speed of light * wavelength
energy of photons (E) = planck's constant (h) x frequency (V)
29
What is planck's constant?
6.626 x 10^-34 Js
30
What happens when an atom absorbs energy?
electrons move into higher levels, entering the excited state, but lose energy by emitting light when they return to their lower level, because the excited state is unstable
31
who created the first accepted version of the periodic table?
Dimitri Mendeleev
32
How did Dmitri Medeleev group elements?
He grouped elements by atomic mass
33
What did Dmitri Mendeleev realize when he grouped his elements?
groups/columns had similar chemical properties
34
What are some properties of metals?
Good conductors of heat and electricity, shiny, and ductile
35
What are some properties of non metals?
poor conductors, not malleable or ductile, brittle, dull
36
What are metalloids?
elements with properties of both metals and nonmetals
37
What is electron shielding?
the blocking of valence shell electron attraction by the nucleus due to the presence of inner shell electrons
38
what is ionization energy?
the amount of energy required to remove an electron from an atom in its gaseous state
39
what is the periodic trend and group trend of ionization energy?
from left to right ionization energy increases, because atomic size decreases. From top to bottom ionization energy decreases, as atomic size increases
40
What is the ionic radius of a cation compared to a neutral atom?
cations are smaller because losing an electron results in more attraction from the nucleus, pulling all of the electrons closing
41
what is the periodic trend and group trend of ionic radius?
left to right, decreases. down a column, increases
42
What is electronegativity?
the ability of an atom to attract electrons
43
what is the periodic trend of electronegativity?
as you move left to right, it increases, and as you move down, it decreases
44
what are covalent bonds?
- sharing of electrons between non-metals
- electronegativity difference < 2.0
- not water soluble
45
What is the electronegativity difference of polar covalent bonds?
> 0.5 < 2
46
what is the electronegativity difference of non-polar covalent bonds?
< 0.5
47
what is an ionic bond?
- occur when an atom transfers electrons to another atom
- bonds between metals and nonmetals
- electronegativity is > 2.0
- called salts or crystals
- water soluble
48
what is a hydrogen bond?
- intermolecular bond
- formed between molecules that have polar covalent bonds
- H-O, H-N, H-F
- the partial positive charge of hydrogen is attracted to the partial negative charge of a different atom
49
What kind of bond does water contain?
polar covalent bonds between oxygen and hydrogen
50
What are the properties of water?
- high melting/boiling point
- ice less dense than water
- cohesion AND adhesion
- surface tension
- universal solvent
51
What is pH?
the measure of the hydrogen ion concentration of a solution
52
What is a buffer?
A solution that resists change in pH by either absorbing excess hydrogen ions or donating them
53
What are the 4 classes of macromolecules?
carbohydrates, lipids, nucleic acids, and proteins
54
what is a monomer?
A single molecule; the building blocks of a polymer
55
what are the monomers and polymers of carbohydrates?
monosaccharides and polysaccharides
56
What are some examples of complex carbohydrates?
* starch (potatoes, peas, corn: can be broken down into glucose for energy)
* glycogen (animals store sugar in the form of glycogen)
* cellulose (structural materials in plants' cell walls and stems),
* whole grains, like breads
* legumes, like beans and lentils.
57
What are the monomers of fat?
fatty acids and glycerol
58
What are phospholipids?
lipids similar to fats but that only have 2 fatty acids
59
What is special about phospholipids?
They have hydrophilic heads and hydrophobic tails that form the bilayer of cell membranes. The tails face each other, and the heads face outwards
60
What is triglyceride (fat) composed of?
3 fatty acid chains and a glycerol
61
What are waxes?
contains one fatty acid linked to a long chain alcohol. more hydrophobic than fats and are found on the coatings for fruits, plants, and insects
62
What are steroids?
carbon skeleton forms four fused rings, found in cholesterol and hormones
63
Where are the monomers of nucleic acids?
nucleotides
64
What are the monomers of proteins?
amino acids
65
What are the 3 parts of a nucleotide?
phosphate, 5 carbon sugar, nitrogenous base
66
What is dehydration synthesis?
Monomers link together to form polymers by losing water
67
what is hydrolysis?
polymers are broken down into monomers using the reverse reaction of dehydration synthesis. They gain water, which breaks bonds
68
What are the 5 functional groups essential to life?
hydroxyl group, carbonyl group, carboxyl group, amino group, and phosphate group
69
What are the monomers and polymers of lipids?
glycerol and fatty acid chains are monomers, triglycerides, steroids, waxes, and phospholipids are polymers
70
What are the differences between saturated and unsaturated fats (triglycerides)?
Saturated - all three fatty acid chains have single bonds, allowing for a maximum number of hydrogen atoms
Unsaturated - one or more fatty acid chains have one or more double bonds.
71
free card :)
:DDD
72
What are lipids?
nonpolar molecules that are not attracted to water - hydrophobic
73
What is the function of carbohydrates?
provide energy
74
What are the functions of lipids?
insulation, cushioning, organs, provide energy
75
What are nucleic acids?
polymers that serve as
the blueprints for proteins
76
What are the two types of nucleic acids?
DNA & RNA
77
What is DNA?
- deoxyribonucleic acid
- Contains genes that sequence amino
acids to code for proteins.
- Double strand
78
What is RNA?
- ribonucleic acid
- Copies information from DNA and
translates it into protein structure.
- Single strand
79
How many different amino acids are there in the human body and how do they differ?
There are 20, and they only have different R (side chain) groups
80
What are the 3 parts of an amino acid?
an amino group (-NH2), a carboxyl group (-COOH), and a side chain (R-group)
81
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82
what is an atom
the smallest part of a chemical element that can exist and still have the element's properties. the building blocks of matter
83
what info do you get from the atomic number
tells how many protons the atom of the element contains, the number of protons in the nucleus of an atom of an element. The atomic number identifies the element.
84
mass number
the total number of protons and neutrons in an atom. to find, round atomic mass to nearest whole number.
OR
(the atomic mass rounded to a whole number)
the total number of protons and neutrons in an atom’s nucleus
85
atomic mass unit (amu)
the unit used to measure the mass of subatomic particles
86
what is percent abundance
the percent makeup of the element by the individual isotopes (ex. C-12 (98.9%), C-13 (1.1%), C-14 (a trace amount)
87
atomic mass
the weighted average mass of all isotopes of the element
88
electron cloud
"massless" electrons circle nucleus billions of times per second
- The location of the electrons in the quantum mechanical model of the atom
89
orbital filling diagram
A diagram that represents and guided electron configuration within orbitals
90
transverse wave
- a wave in which particles of the medium vibrate perpendicular to the direction that the wave travels.
- The high points are called crests, and the low points are called troughs.
- S waves are transverse waves that travel through underground rocks during earthquakes
91
photon
- tiny, particle-like bundles of radiation
- absorbed and released by electrons
- energy increases with wave frequency
92
What elements are in the Hydroxyl group?
Hydrogen and Oxygen
93
What elements are in the carbonyl group?
Carbon and Oxygen
94
What elements are in the carboxyl group?
Carbon, oxygen, and hydrogen
95
What elements are in the amino group?
Hydrogen and Nitrogen
96
What elements are in the phosphate group?
Phosphate and Oxygen
