JLH Chem 2nd pp Flashcards
(147 cards)
1
Q
Elements
A
pure substances
can’t be broken down to a simpler pure
substance by a chemical reaction.
Most are naturally occurring
2
Q
Most elements are monoatomic. What does this mean?
A
Only 1 atom
(noble gases are all monatomic)
3
Q
Some elements are polyatomic. What does this mean?
A
contains more than one atom
Examples: N2, Cl2, O2, O3, S8, diamond
4
Q
Element names for:
Copper
Gold
Iron
A
Copper: Cu
Gold: Au
Iron: Fe
5
Q
Element names for
Lead
Mercury
Potassium
A
Lead: Pb
Mercury Hg
Potassium K
Potassium K
6
Q
Element names for
Silver
Sodium
Tin
A
Silver: Ag
Sodium: Na
Tin: Sn
7
Q
What 4 elements are called the building block elements since they make up 96% of living organisms?
A
Carbon (C)
Oxygen (O)
Nitrogen (N)
Hydrogen (H)
8
Q
What are the Major minerals (macronutrients)?
A
Potassium (K)
Phosphorus (P)
Sodium (Na)
Sulfur (S)
Chlorine (Cl)
Calcium (Ca)
Magnesium (Mg)
Make up .1-0.2% of elements
9
Q
Trace elements (micronutrients)
A
Copper (Cu)
Fluorine (F)
Iodine (I)
Iron (Fe)
Nickel (Ni)
Zinc (Zn)
and more
10
Q
Compound
A
formed when you chemically combine two or more elements
NaCl
H2O
C8H18
C8H18
11
Q
Atom
A
smallest basic unit of an element
12
Q
What are the 3 subatomic particles?
A
Protons
Neutrons
Electrons
The quantities and location of these subatomic particles in the atom are responsible for the properties of the element
13
Q
Protons (p)
A
Positive 1 charge
Mass of 1 amu (atomic mass unit)
Located in nucleus
Defines the element (each element has a different # of protons)
14
Q
Neutron
A
No charge
Mass of 1 amu
located in the nucleus
acts as “atomic glue”, keeping nucleus together (protons repel each other)
15
Q
Electron (e-)
A
Negative 1 charge
about 2000x smaller than p & n
located in electron cloud that surrounds nucleus
responsible for chemical reactions & balancing proton charge
16
Q
Why do the electrons move around the nucleus?
A
The negatively charged electrons are attracted to the positively charged protons (opposites attract).
17
Q
What is the comparative size between the nucleus and electron cloud?
A
The nucleus is very small compared to the electron cloud.
If the nucleus was a marble, the atom would be the size of the Superdome!
18
Q
Atoms are tiny (~1 x 10^-24 g) and can’t be measured directly by instruments. We measure mass relative to one another using what as a reference?
A
Carbon-12 (C-12)
1 atomic mass unit (amu) is equal to exactly 1/12 the mass of a C-12 atom.
19
Q
1 amu =
A
1.66x10^-24 g
Protons and neutrons both have masses of ~ 1 amu.
20
Q
An element has a given number of what in each atom?
A
Protons
All C atoms have 6 protons, All H atoms have 1 proton, etc.
21
Q
(Z number)
A
Atomic number
the number of protons in an atom
22
Q
Mass number (A)
A
protons + neutrons
23
Q
What can we determine if we have both the Z number and A number?
A
Can determine number of protons, neutrons and electrons
number of e─ = number of protons
24
Q
All elements of an atom have same number of what?
A
protons
25
Can the number of neutrons vary?
yes.
This is why we have isotopes.
* Uranium isotopes*
* Both have 92 protons*
26
How similar are isotopes usually?
Generally the properties of isotopes are identical.
*Sometimes one isotope is radioactive.*
27
Sometimes one isotope is radioactive.
Used as diagnostic tool and for medical treatments
I-131 (iodine 131)
28
How is the mass of molecules calculated?
calculated by adding masses of individual atoms
H2O:
2H= 2(1.008amu) +
O= (16.00amu) =
18.02 amu
29
Groups of periodic table
**vertical columns**
*(these elements have similar properties)*
30
**main group elements**
*(representative elements)*
the elements in groups 1, 2, and 13 through 18 of the periodic table
31
Transition metals
groups 3-12
32
inner transition elements
lanthanides and actinides ![]()
33
nonmetals on the periodic table
elements to the right of metalloids
34
metalloids
Elements that have properties of both metals and nonmetals.
35
some characteristics of metals
Shiny
Good conductors
Mostly solids
Give up electrons to form compounds with non-metals
36
some characteristics of non-metals
Not shiny
Not good conductors
Often polyatomic
Solids liquids and gases
Take additional electrons to form compounds with metals or "share electrons" with other non-metals
37
some characteristics of nobel gases
Monoatomic
Unreactive
38
Electron clouds are not random. Explain a little more.
Electrons confined to specific area
Discreet energy levels
39
What are the shells of an atom?
Specific energy levels
n= 1,2,3,4 etc.
*The path of an electron around the nucleus of an atom (orbit)*
40
What shells fill first?
lower shells
41
What are shells broken down into?
subshells
s, p, d, f
42
Each subshell contains what?
orbitals
43
How many electrons can an orbital have?
2 max
44
Electron configuration
1s 2s 2p 3s 3p
45
What do we use to determine total electrons?
Z (atomic number)
46
Fe has 26 electrons. What is the electron configuration?
1s2
2s2
2p6
3s2
3p6
4s2
3d6
47
What is the maximum number of valence electrons?
8
*except H & He- max is 2*
48
Periodic trend
properties that change in a regular way across a row or down a column
49
Ionization Energy
The energy needed to remove an electron from a neutral atom
50
Electronegativity
the ability of a **bonded atom** to pull the electrons toward it.
Think of it as the attraction between the nucleus and the valence electrons.
51
Both ionization energy and electronegativity are a measure of the atom's ability to do what?
hold on to it's electrons.
52
Metals on left side of chart
Low ionization energy/electronegativity.
Few "dots".
Easier to give up 1 or 2 electrons than gain 6 or 7.
This explains why metals give up electrons to form compounds
53
Non-metals on the right
High Ionization energy/electronegativity.
High number of "dots"
Easier to take a couple of electrons than to give up a bunch.
This explains why non-metals take electrons to form compounds.
54
Atomic size
distance between nucleus and outer edge of valence shell
Increases as you go down periodic chart.
Number of electrons increasing so more shells
Decreases as you go from left to right.
Atoms toward right are holding the electrons tighter (leading to smaller radius)
55
How many elements are currently known?
118 elements
56
How many elements are naturally occurring?
90 elements are naturally occuring
*28 have been prepared by scientists in a lab*
57
Carbon Monoxide (CO) is formed in small amounts during what?
combustion of fossil fuels like gasoline.
*CO: Carbon and oxygen*
58
what is Rn?
**Radon** (noble gas)
*radioactive gas produced in the soil*
59
what is the main component of the earth's atmosphere?
Nitrogen (N)
60
3 categories of periodic table
metals, nonmetals, metalloids
61
All metals are solid at room temperature except what?
mercury (liquid)
62
what non-metal is liquid at room temperature?
Bromine
63
What are the 7 metalloids?
Boron (B)
Silicon (Si)
Germanium (Ge)
Arsenic (As)
Antimony (Sb)
Tellurium (Te)
Polonium (Po)
***bor**ing **sil**ly **germ**s **are** **ant**s **tell**ing **pol**itics*
64
What are the elements that form water?
Oxygen and Hydrogen
65
What elements are found in the proteins, carbs, lipids, and nucleic acids?
Carbon
Hydrogen
Oxygen
*nitrogen is found in proteins & nucleic acids*
66
What macronutrients are found in our body fluids?
Potassium
Chlorine
Sodium
67
What macronutrient is found in all nucleic acids?
Phosphorus
68
At least how much of each macronutrient is needed in the daily diet
100 mg of each
69
Trace elements (micronutrients) are needed in the daily diet in small quantities, usually less than what?
15mg
70
2H2 + O2 → 2H2O
Coefficients (2) & subscripts (2)
71
What color sphere is used for the element oxygen?
Hydrogen?
O2: Red
H: Gray
72
What color sphere is used for the element Carbon?
Nitrogen?
C: Black
N: Blue
73
What color sphere is used for the element Chloride?
fluorine?
chloride (Cl): green
fluorine (F): yellow
74
What elements are in NaCN?
1 sodium (Na)
1 carbon (C)
1 nitrogen (N)
75
All matter is composed of the same basic building blocks called what?
atoms
76
most of the mass of an atom resides where?
nucleus
77
what comprises most of the volume of an atom?
electron cloud
78
because the mass of an individual atom is so small, chemists use a standard mass unit called what?
Atomic mass unit (amu)
79
What is the isotope hydrogen, with one neutron and one proton (mass number=2), called?
Deuterium (D)
80
What is the isotope hydrogen with a mass number = 3 called?
tritium (T)
81
Determine the number of neutrons in the isotope carbon-14
Since carbon's atomic number (Z) is 6 we just subtract 6 from 14 = 8 neutrons
82
How do we determine the atomic weight of isotopes?
1: find amu of each & their abundance (75.78%)
2: multiply amu by percent (for each)
3: add the answers
83
What is the atomic weight of copper:
**_2 isotopes_**
copper-63 (62.93 amu, 69.17%)
copper-65 (64.93 amu, 30.83%)
63.546 u
84
iodine-131 is used for
thyroid disease
85
iodine is a micronutrient needed by the body to synthesize what?
thyroxine
(thyroid hormone)
*contains 4 iodine atoms*
86
To evaluate the thyroid gland, a patient can be given sodium iodide (NaI) that contains radioactive iodine-131. Iodine-31 is taken up in the thyroid gland & as it emits radiation, it produces an image in a thyroid scan.
87
who created the periodic table?
Dmitri Mendeleev (1869)
88
Elements in the same row (period) in the periodic table are similar in what way?
size
89
A column in the periodic table is called a group. What do elements in the same group have similar?
similar electronic & chemical properties
90
How many rows are on the periodic table?
7
91
what do the lanthanides begin with?
**Cerium** (Z=58)
*after lanthanum (La)*
92
what do the actinides begin with?
Thorium (Z=90)
*after actinium (Ac)*
93
What is 1A-8A groups?
1, 2, & 13-18
(main groups)
94
what is 1B-8B?
3-12
(transition metal elements)
95
Alkali metals are in group 1A. Hydrogen is in group 1A, is it an alkali metal?
no
96
What are the alkali metals?
Lithium
Sodium
Potassium
Rubidium
Cesium
Francium
*Like some pork roast cooked fresh*
97
characteristics of alkali metals
soft, shiny, low melting points
good conductors
react readily with water to form basic solutions
98
What are alkaline earth metals?
Beryllium
Magnesium
Calcium
Strontium
Barium
Radium
*buried magazines can still be read*
99
None of the metals in groups 1A & 2A exist in nature as pure elements; rather, they are always combined with other elements to form compounds. What are some examples of compounds formed from 1A?
NaCl
KI (potassium iodide)
100
None of the metals in groups 1A & 2A exist in nature as pure elements; rather, they are always combined with other elements to form compounds. What are some examples of compounds formed from 2A?
Magnesium sulfate (MgSO4)
barium sulfate (BaSO4)
101
what are the halogens?
fluorine (F)
Chlorine (Cl)
Bromine (Br)
Iodine (I)
Astatine (At)
*find chief Brom in Alaska*
102
In their elemental form, halogens contain what?
2 atoms joined together
Cl2, Br2, & I2
103
Are halogens reactive?
very reactive
combine with many other elements to form compounds
104
what halogens are gases at room temperature?
fluorine
chlorine
105
which halogen is liquid at room temp?
bromine
106
what halogen is solid at room temp?
iodine
107
what are the noble gases?
helium (He)
Neon (Ne)
Argon (Ar)
Krypton (Kr)
Xenon (Xe)
Radon (Rn)
*he'll need Argon, Krypton, Xenon & Radon*
108
How do elements in a group of the periodic table have similar chemical properties?
The chemical properties of an element are determined by the number of electrons in an atom.
109
the modern description of the electronic structure of an atom is based on what principles?
Electrons do not move freely in space; rather, an electron is confined to a specific region, giving it a particular energy.
Electrons occupy discrete energy levels. The energy of electrons is quantized; that is the energy is restricted to specific values.
110
The electrons that surround a nucleus are confined to regions called what?
principal energy levels or shells
*1s*
111
The number of electrons that can occupy a given shell is determined by what?
value of n
112
The farther a shell is from the nucleus, the ______ its volume becomes, and the ____ \_\_\_\_\_\_\_\_\_ it can hold.
The farther a shell is from the nucleus, the **larger** its volume becomes, and the **more electrons** it can hold.
113
how many electrons can the first, second and third shells hold?
1st: 2
2nd: 8
3rd: 18
* max # of e- is given by the formula 2(n^2)*
114
Orbital
region of space where the probability of finding an electron is high.
*Each orbital can hold 2 electrons*
115
The two electrons in an orbital must have ________ spins.
The two electrons in an orbital must have opposite spins.
116
A particular type of subshell contains a specific number of orbitals. How do we figure out how many orbitals each subshell contains?
S = l-0
P = l-1
D = l-2
F = l-3
l-0 = 0 (1 orbital)
l-1 = -1, 0, +1 (3 orbitals)
l-2 = -2, -1, 0, 1, 2 (5 orbitals)
l-3 = -3, -2, -1 0, 1, 2, 3 (7 orbitals)
117
The first shell of electrons around a nucleus (n=1) has only one s orbital, called the 1s orbital because it is in the first shell. What (type of) orbitals does the 2nd shell of electrons have?
**_2 types:_**
1 s orbital (2s)
3 p orbitals (2px, 2py, 2pz)
*called 2s & 2p orbitals because they are located in the second shell.*
118
The 3rd shell of electrons (n=3) has how many orbitals?
3 types:
1 s orbital
3 p orbitals
5 d orbitals
*(3s, 3p, 3d)*
119
The maximum number of electrons that can occupy a shell is determined by what?
the number of orbitals in the shell.
120
Shapes of orbitals
**_s orbital:_**
sphere
**_p orbital:_**
peanut
**_d orbital:_**
donut
121
All s orbitals are spherical, but what happens when the shell number increases?
the orbital gets larger
122
The 3 p orbitals in a shell are what to each other along the x, y, & z axes?
perpendicular
123
What is the lowest-energy arrangement of electrons called?
ground-state
124
What are 3 rules to determine the ground-state electronic configuration of an atom?
1) electrons are placed in the lowest-energy orbitals beginning with the 1s orbital
2) Each orbital holds max of 2 electrons
3) When orbitals are equal in energy, one electron is added to each orbital until the orbitals are half-filled, before any orbital is completely filled.
125
orbital diagram
box = orbitals
arrows = electrons
126
In an orbital diagram, a single electron is called what?
unpaired electron
(single arrow pointing up)
127
the 4s orbital is filled with electrons before the 3d orbitals because it is lower in energy.
4s = 4+0 = 4
3d = 3+2 = 5
128
What does the orbital diagram for Hydrogen look like?
Helium?
Hydrogen: 1s^1
(shell 1, s subshell, 1 electron)
Helium: 1s^2
(shell 1, s subshell, 2 electrons)
129
Lithium has 3 electrons on period 2, group 1. how many electrons are in the ground state?
2 electrons are in the 1s orbital.
The remaining electron is an unpaired electron in the 2s orbital
1s2 2s1
130
Oxygen has 8 electrons. In the ground state, 2 electrons are added to both the 1s & 2s orbitals. The remaining 4 electrons must be distributed among what?
the 3 2p orbitals to give the lowest-energy arrangement.
131
How can we shorten the electronic configuration for carbon from 1s2 2s2 2p2?
He 2s2 2p2
use the name of the noble gas from the preceding row and add the remaining orbitals & subscripts
132
What groups does the s block consist of?
groups 1A & 2A & helium
133
What groups does the p block consist of?
groups 3A-8A (except helium)
134
What does the d block consist of?
the 10 columns of transition metals
135
What does the f block consist of?
The 2 groups of 14 inner transition metals.
136
how do you draw an orbital diagram for the ground-state electronic configuration of sulfur?
Use Z # to determine # of electrons (16)
Locate element in PTable
+ 2 electrons to each of the 1s, 2s, three 2p, & 3s orbitals (12 electrons used)
for last 4 e-
give one orbital 2 electrons & place one unpaired electron in the remaining two orbitals
137
What is the electronic configuration for sulfur (orbital diagram)?
Remember, when you get to the p subshell it has 3 orbitals and each one gets one electron before any get 2.
When looking at the periodic table you can look at a pair of elements as an orbital (Al & Si = 1 orbital). You can also look at each element as one space for one electron (Al would be where you would put a single electron-\> up pointing arrow.) You would skip Si and put your next unpaired electron in P. After P you would go to Cl then you would go back to Si then S then Ar.
138
draw an orbital diagram for:
Magnesium
Aluminum
Bromine
139
The chemical properties of an element depend on what electrons?
most loosely held (valence)
(period number tells the number of shells;
group number tells # of valence e-)
140
The chemical properties of a group are similar because these elements contain the same what?
electronic configuration of valence electrons
141
what is the total number of electrons, valence electrons, & name of the element:
1s2 2s2 2p6 3s2 3p2
Si
14 electrons
1s2 2s2 2p6 3s2 3p2
highest shell is 3
valence electrons are in highest shell
2 + 2 = 4 V electrons
142
Electron-dot symbol
(Lewis dot structure)
for 1-4
v electrons, single dots are used.
With more than 4 electrons, dots are paired
143
What are 2 properties that illustrate periodic trends?
atomic size
ionization energy
144
Removing an electron from a neutral atom forms what?
cation
*ionization energy is the energy needed to remove an electron from a neutral atom*
145
In the same group, what happens with atomic number and atomic radius as we move down the column?
both increase moving down column
146
Does ionization energy decrease or increase moving down the column?
ionization energy decreases moving down a column
147
atom A is smaller than atom B.
If both atoms are in the same period, which atom has the higher atomic number?
atom A (smaller atom)
*because atoms get smaller from left to right and there are more protons moving from left to right on the periodic table.*
