Chapter 2 Flashcards
1
Q
Sub-shell types
A
S, P, D, F
2
Q
S sub-shell has
A
1 orbital that can hold 2 electrons
3
Q
P sub-shell has
A
3 orbitals that can hold 6 electrons
4
Q
D sub-shell has
A
5 orbitals that can hold up to 10 electrons
5
Q
F sub-shell has
A
7 orbitals that can hold up to 14 electrons
6
Q
The atomic number identifies
A
The number of protons & electrons
7
Q
The atomic mass is the
A
Number of protons & neutrons in an atom (sum & is an integer)
8
Q
The group number identifies the
A
Number of valence electrons
9
Q
The period number identifies
A
The number of energy levels
10
Q
What is matter?
A
Anything that has mass & takes up space & does not need to be visible
11
Q
What is the basic building block of matter?
A
Atoms
12
Q
Atoms can join to form
A
Molecules
13
Q
An element
A
Contains only a single kind of atom
14
Q
Compounds contain
A
2 or more kinds of atoms in a fixed ratio
15
Q
Atoms are comprised of
A
Protons, neutrons & electrons
16
Q
Protons are
A
Positively charged
17
Q
The number of protons is also called the
A
Atomic number & determines the identity of the atom
18
Q
Neutrons are
A
Neutral
19
Q
Electrons are
A
Negatively charged
20
Q
Ions are
A
Atoms or a group of atoms bonded together that have a net electrical charge; charge is obtained by adding or subtracting electrons
21
Q
Molecules are a
A
Group of atoms chemically bonded together into a discrete unit by covalent bonds & are electrically NEUTRAL
22
Q
Ionic compounds contain
A
Positively charged ions & negatively charged ions
23
Q
Ionic compounds are
A
Not molecules
24
Q
Physical change occurs
A
Without changing the chemical makeup of the substance undergoing the changes (ex;melting)
25
Chemical changes always result in the formation of
Chemically different substances
26
A physical property can be
Observed or measured without changing the chemical makeup of the substance
27
Which 2 categories do physical properties fall under?
Intensive & Extensive
28
What is Intensive property
Is integral to the material, regardless of how much material there is
ex: color
29
What is Extensive property?
depends on the sample size
ex: volume & mass
30
A chemical property describes
Describes the type of chemical change the material tends to undergo
ex: gases are flammable
31
What are pure substances?
materials that cannot be physically separated into simpler components
32
A substance can either be a
Compound or Element
33
If a substance is a compound, then
It can be chemically separated into its elemental components
34
Mixtures are comprised of
2 or more pure substances
35
Mixtures can be
Resolved into simpler components through physical processes
36
Homogeneous mixtures are
Uniform in chemical & physical properties throughout the sample
ex: NS & Air
37
A heterogeneous mixture exhibits
Distinct phase boundaries between its components
ex: Emesis
38
A phase boundary is
A demarcation where the chemical &/or physical properties of the sample change
39
Can a substance be both a molecule & an element?
Yes
40
Electrons are bound to the nucleus by
The electromagnetic force (attraction of opposite charges)
41
When protons & neutrons combine to form an atomic nucleus,
There is a mass deficit because some of the mass is converted into a binding energy
42
The mass number can
NEVER be smaller than the atomic number
43
Elements are always
Electrically neutral
44
The number of electrons is
Equal to the number of protons in an electrically neutral atom
45
Isotopes have
The same atomic number but a different mass number -or- the same number of protons & a different number of neutrons
46
Compounds are formed by
Bonding atoms together in a fixed ratio
47
Chemical reactions do not
Create, destroy, or change atoms into atoms of other elements; chemical reactions cause atoms to recombine into new substances
48
What is the law of conservation of mass?
No detectable change in the total mass occurs during chemical reactions; during a chemical change, the components of a system are neither created nor destroyed; they simply recombine into new substances
49
What the is law of definite proportions?
Different samples of a pure compound always contain the same elements in the same proportion by mass
50
What is the Law of Multiple Proportions?
Some elements can combine to give more than one compound
51
Elements must be delivered as
Particles (i.e., atoms) rather than a continuous substance
52
How are elements listed on the periodic tabel?
In order of increasing atomic number
53
Vertical columns are called
Groups/Families
54
Elements in a given group have similar
Chemical & physical properties
55
Noble gases are
Colorless, odorless & are extremely reluctant to combine with other elements to form compounds
56
Each row is called a
Period
57
Periods represent adding electrons to
Quantum energy levels in the atom, which are called electron shells
58
Atoms with filled electron shells are
Stable
59
Accepting additional electrons is called
An Anion (negative charge)
60
What are the atomic weights?
Are weighted averages of the atomic masses of the naturally occurring isotopes of that element
61
Characteristic of metals on the periodic table
Shiny luster
Ductile
Malleable
Good Conductors
React chemically to form cations by giving away electrons
62
Nonmetals tend to form
Anions & are brittle
63
What is a well-known semi-conductor?
Silicon
64
Most elements are
Solids under normal conditions
65
Molecular compounds are comprised of
Only nonmetals
66
Ionic compounds are almost always comprised of a
Metal & a nonmetal
67
What is an ion?
An atom or a group of atoms with a charge
68
Ionic compounds consists of ions & are
Held together by ionic bonds, or the attraction of the oppositely charged ions
69
In the solid state, ionic compounds form
Crystalline lattices, in which all the cations are attracted to all the neighboring anions
70
Ionic compounds are sometimes referred to as
Salts
71
A salt is produced by
The reaction of an acid & a base
72
Representative metals almost always form
Cations in which the ionic charge equals the group number
73
Most transition metals
Form more than one cation
74
Polyatomic ions are formed from
2 or more nonmetal atoms that are bonded together in a way that results in a net electrical charge
75
Compounds must be
Electrically neutral
76
The net charge on an ionic compound must be
Zero
77
Compounds that have a strong tendency to absorb water are called
Hygroscopic
78
The anhydrous form of a compound that has a strong tendency to absorb water can
Be used as a desiccant
79
Desiccants scavenge the last
Traces of water from a system
80
Electricity is described as the
Flow of charged particles under the influence of an electric field
81
An electrolyte is a
Substance that dissolves in water to give a solution that conducts electricity
82
A nonelectrolyte is a
Substance that dissolves ion water to give a solution that does not conduct electricity
83
Molecular compounds are
Nonelectrolytes, unless they have acid or base properties
84
When ionic compounds dissolve in water, they mostly
Separate into ions that freely & independently move around; the solution will conduct electricity
85
Water is a
nonelectrolyte
86
Water is a molecular substance because
It is a compund of nonmetals
87
Pure water is a
Nonelectrolyte & is a very poor conductor of electricity
88
Stoichiometry includes
The calculations that relate amounts of reactants & /or products in a chemical reaction
89
Moles are a quantity of material, analogous toa dozen & is the
Amount of substance that contains exactly as many particles as there are in exactly 12g of carbon-12
90
Mole number is often called
Avogadro's number thats equal to 6.02 x 10 to the 23
91
The molar mass of an element is equal to
Its atomic mass
92
For molecules, the molar mass is
Equal to the sum of the masses of the component atoms
93
Where is the mass number/atomic mass number located?
The bottom number in the periodic taable
94
What are isotopes?
Same number of protons but different number of neutrons
95
What are the outermost shells of electrons called?
Valence electrons
96
What is involved in molecular bonding?
The valence electrons
97
Molecular bonding may occur
By direct sharing of electrons or by thermodynamic interaction
98
What are the 2 types of bonds?
Covalent & Electrostatic
99
What is it called when atoms of differing elements bond?
Compounds
100
The physical sharing of electrons between atoms is called a
Covalent bond
101
What are stronger than electrostatic bonds?
Covalent Bonds
102
Electrostatic bonding may include
Ion-Ion
Ion-Dipole
Dipole- Dipole
103
Which is the strongest electrostatic bond?
Ion to Ion
They are not directions & occur anywhere
104
Molecules with ionic bonds have
Higher melting & boiling points
105
Ion to dipole bonds only have
Partial charges
106
An uneven distribution of charges creates a
Dipole
107
Which is the weakest of ALL molecular bonds?
London forces
108
Lewis structures are
Dots or lines that show valence electrons; only the outer shell is depicted
109
What are isomers?
Molecules that have the SAME chemical formula but DIFFERENT structures
110
What is the same in isomers?
The number & type of atoms & bonds, but the arrangement of the atoms are different
111
Isomers can be
Structural or Stereoisomers
112
What are structural isomers?
Have the same molecular formula, but their atoms are located in different places
113
Structural isomers are truly
Different molecules with differing physical & chemical properties
114
What are stereoisomers?
Have similar geometric arrangement of atoms but differ in their spatial position
115
Stereoisomers can be
Enantiomers or Diastereomers
116
What are enantiomers?
Mirror images of one another & CANNOT BE superimposed
Have similar chemical & physical properties
Optically active & can rotate polarized light in a clockwise fashion (+/dextro) or counterclockwise (-/leva)
117
What are diastereomers?
NOT mirror images & may have differing physical & chemical properties
118
What is bond energy?
The amount of energy needed to make or break a bond
119
Energy is released when
A bond is formed
120
Energy is consumed when
A bond is broken
121
What possess greater bond energy?
Short bonds like covalent bonds
122
What happens when molecular bonds are broken?
New molecular bonds are formed & energy is released
123
Bond energies are measured as
An enthalpy change
124
What is Enthalpy?
The total amount of energy possessed by a system (system can be on an atomic or macroscopic scale)
125
The Enthalpy of a system is the
Total of all kinetic & potential energy
The stored/potential energy includes its height in relation to the force of gravity & the energy stored in the bonds of its molecules, atoms & even subatomic particles
126
Change of energy is
Easier to measure rather than total energy (enthalpy)
127
What is mass?
Total of all matter in an object- the sum of the mass of all the electrons, protons & neutrons
128
What is weight?
The total effect of gravity pulling on all the electrons, protons & neutrons
129
What is a Dyne?
1/1000 of a newton
The force required to move 1g of weight 1cm/sec
130
When are Dynes used
To calculate SVR & PVR
131
An EKG is an example of a
Vector
132
Mass Spectrometry is used
In anesthetic gas analysis
(ionized gas molecules)
133
Identification of a gas is based on
The amount of deflection
134
