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Chemistry Quiz 1 > Chapter 2 > Flashcards

Chapter 2 Flashcards

1
Q

Symbol

A

The abbreviation for an element consisting of a capital letter (may also be followed by a lower letter)

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2
Q

Formulas

A

A combination of symbols, subscripts, and possible superscripts that identifies the composition of an element, compound, or ion

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3
Q

Why are symbols combined?

A

Chemists write chemical symbols together in chemical formulas to identify compounds

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4
Q

What do formulas tell about each element?

A

Formulas give the relative number of each type of element in a compound

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5
Q

Subscripts

A

In chemical formulas to indicate the relative proportions of the elements present

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6
Q

What letters are capitalized in a symbol?

A

The first letter in a symbol is the only letter to be capitalized

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7
Q

Do all symbols start with the same letter as the English name?

A

No

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8
Q

How are compounds represented?

A

Compounds are represented by the combination of chemical symbols in chemical formulas

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9
Q

The law of conservation of mass

A

During a chemical reaction mass is neither gained nor destroyed

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10
Q

Explain the law of conservation of mass

A
  • During a chemical reaction mass is neither gained nor destroyed
  • it is converted into different states of matter but not lost or gained
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11
Q

What are the two laws the conservation of mass lead to?

A
  1. Law of definite proportions (law of constant composition)
  2. Law of multiple proportions
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12
Q

Law of definite proportions

A

The composition of a compound is fixed

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13
Q

Proportion

A

the ratio of the number of a certain item divided by the total number of items (compare to percent)

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14
Q

What is the proportion of mass in a compound?

A

The proportion of mass of an element in a compound is the ratio of the element to the total mass of the compound

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15
Q

Percent

A

The amount of a certain component in 100 units of the atom

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16
Q

What is the percent by mass of an element?

A

The percent by mass of the element in the compound Is just the proportion of the element multiplied by 100

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17
Q

The law of multiple proportions

A

Two or more elements combine to form more than one compound, for a fixed mass of one element, the masses of each of the other elements in the compounds occur in a small whole-number ratio

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18
Q

What led to the development of the law of conversation of mass?

A

Careful measurement of the masses of reactant and products in chemical reactions led to the development of the laws of conservation of mass, definite proportions, and multiple proportions

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19
Q

Why are the three laws important?

A

The three laws of chemical composition formed the basis for the theoretical development of chemistry

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20
Q

Daltons Atomic Theory

A

The theory that matter is mate up of small particles that have properties characteristic of an element

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21
Q

Dalton’s atomic theory hypothesis

A
  1. Matter is made up of tiny, indivisible particles called atoms
  2. Each atom of a particular element has the same mass but the mass of an atom of one element is different from the mass of an atom of any other element
  3. Atoms combine to form what we now call molecules. When they do so, they combine in small whole number ratios
  4. Atoms of some pairs of elements can combine with each other in different small whole-number ratios to form different compounds
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22
Q

Atoms

A

A single particle of any elements - the smallest possible amount of an element that retains the properties of that element

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23
Q

Molecules

A

An uncharges, covalently bonded group of atoms

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24
Q

What three things did Dalton’s atomic theory explain

A
  1. The law of conservation of mass
  2. The law of definite proportions
  3. The law of multiple proportions
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25
Cathode rays
A beam of electrons
26
How were electrons discovered?
- Constructed a cathode rube and observed how a beam of particles known as a cathode ray passed through the tube - discovered they have a negative charge because they bent away from a magnet - cathode rays move in straight lines - have a charge to mass ratio of -1.76x10^8 C/g (coulomb)
27
Electrons
A negatively charged subatomic particle found outside the nucleus, a fundamental particle of nature
28
Charge of an electron
-1.60x10-19 C
29
Mass of an electron
9.10x10^-28
30
Radioactivity
the emission of particles during nuclear decay
31
Three types of radioactivity
1. Alpha 2. Gamma 3. Beta`
32
Rutherfords Model
1. The atom has a positive charge and the majority of its mass are located in a relatively small area, which he later names the nucleus 2. the majority of the atom is empty space. Small, negatively charged electrons are spread throughout this empty space 3. The number of negatively charged electrons is equal to the number of positively charged protons inside the nucleus
33
Nucleus
The center of the atom, consisting of the protons and neutrons. It accounts for almost all of the mass, but almost none of the volume of an atom
34
Proton
A subatomic particle found in the nucleus with a mass slightly greater than 1u and a charge of +1
35
Neutrons
A subatomic particle sound in the nucleus that has no charge and a mass slightly greater than 1u
36
Charges on PNE
proton = +1 Electron = -1 Neutron = no charge
37
Why is daltons atomic theory important?
Daltons atomic theory was an explination for why the three laws of chemical combination worked, and it provided the theoretical background for the entire future development of chemistry
38
How were the atom's parts found?
Experiments demonstrated that the atom is not indivisible but consists of a nucleus made up of protons and neutrons that us surrounded by a cloud of electrons
39
Explain the charges on an atom
The charges on protons and electrons are equal in magnitude and atoms are electrically neutral so atoms contain equal numbers of protons and electrons
40
Subatomic particles
A proton neutron or electron
41
What is the size of the nucleus
The nucleus is 1/10000 the size of the radius of an atom
42
Neutral
neither negatively or positively charged
43
Atomic number
- Z Number of protons in the nucleus of each atom of an element
44
The number of protons equals ____
the number of electrons
45
Isotopes
A form of an element whose atoms have the same number of protons but different numbers of neutrons
46
How are isotopes related to elements?
Isotopes are still the atoms of the same element because they have the same atomic number but different numbers of neutrons
47
Mass number
- A - The sume of the number of protons and the number of neutrons in an atom
48
Mass Number and Atomic Number overview
- Atomic number (z) = number of protons - Mass Number (A) = P + N
49
Ions
An atom or group of atoms that has gained or lost electrons therefore has a net negative or positive charge
50
Cations
A positively charged ion
51
Anions
A negatively charged ion
52
What are atoms composed of?
Atoms are composed of subatomic particles: protons (p) neutrons (n) and electrons (e)
53
Explain the diagram of the atom
- Protons and neutrons are found in the nucleus and account for essentially all of the mass of the atom. - Protons are positively charged - Neutrons and electrically neutral
54
What is the Mass Number (A)
The total number of protons and neutrons in the atoms
55
Explain electrons
Electrons are found outside the nucleus and make up essentially all of the volume of the atom, electrons are negatively charged
56
What is the Atomic Number?
The atomic number (z) is equal to the number of protons in the nucleus and determines which element the atom is identified as
57
What atoms are isotopes?
Atoms with different numbers of neutrons but the same number of protons are isotopes of each other
58
When are ions formed?
Ions are formed when an atom gives or loses electrons
59
Different types of ions
Positively charged ions are called cations, while negatively charged ions are called anions
60
Relative Scale
A scale based on an arbitrary chosen standard
61
Atomic mass scale
A relative scale of masses based on the mass of carbon-12 being the standard and having a mass defined as exactly 12 u
62
Atomic mass units (amu)
- A mass equal to one-twelth of the mass of a carbon-12 atom - replaced with a new standard that is based on the mass of a single carbon isotope
63
u to gram
6.022x10^23 u = 1.00 g
64
The modern determination is mass
- Modern method of determining atomic mass uses C isotope as the standard - mass of a single C atom is 12u - weighted average
65
Atomic mass
the weighted average of the masses of the naturally occurring mixture of isotopes of an element, compared with one-twelfth of the mass of a carbon 12 atom
66
Weighted average
the average volume of several types of items, taking into account the number of individual items od each type
67
Atomic mass formula
Atomic Mass = Fraction of isotope x mass of isotope
68
Atomic mass definition
naturally occuring mixture of isotopes
69
What does mass number refer to
an individual isotope
70
Explain atomic mass's relativity
Atomic mass would be different on another planet because the natural abundances would be different
71
Explain the development of atomic mass
historically, atomic mass was determined from mass ratios such as those used to develop the law of opposite proportions. Today the mass and percent occurrence of each isotope are used
72
Atomic mass vs Mass Number
Atomic mass is the weighted average of the masses of the naturally occurring mixture of isotopes of an element. Do not confuse the atomic mass with the mass Number, which is the total number of protons and neutrons in the atom
73
Periodic Table
An organization of elements by increasing atomic number with elements having similar chemical properties aligned in vertical columns
74
Horizontal rows on the periodic table
arranged in increasing atomic numbers (z)
75
Vertical columns on the periodic table
elements with similar chemical properties
76
Noble gases
colorless, odorless gases and almost totally inert
77
What is special about noble gases
discovered after the periodic table was first formulated - lack of combining means they are not found in any naturally occurring compounds
78
period
one of the seven hirozontal rows
79
group
in the periodic table a column that includes elements with similar chemical properties
80
alkali metals
a metal in group one
81
Alkaline earth
a metal in group two
82
coinage metals
copper silver and gold
83
halogens
an element in periodic group 7
84
noble gases
an element in the far right column of the periodic table
85
main group elements
elements in group 1, 2, 13-18
86
transition metals
any element in groups 3-12 having atomic numbers 21-30, 39-48, 57, 72-80, or 104-112 and designated with B in the classical group naming system
87
innertransition elements
a collective term for the lanthanoids and actinoids
88
post transition elements
group 12 (2B)
89
Metals
an element on the left of the stairste[ line in the periodic table or a mixture of such elements
90
How to classify a metal
- solid at room temperature - conduct heat and electricity - maliable - ductile
91
nonmetals
Hydrogen or any other element to the right of the stairstep line in the periodic table
92
How to classify nonmetals
- many are gases at room temp - brittle - nonconductive
93
metalloids
An element near the stairstep line between metals and nonmetals
94
How to classify metalloids
- some properties of metals and nonmetals
95
How was the original periodic table developed?
The periodic table was originally developed using atomic masses and the chemical and physical properties of the elements but it is now known that atomic numbers not masses are the basis for the properties of an element
96
How is the modern periodic table organized
The modern periodic table is organized in order of increasing atomic number
97
Why is the organization of the periodic table important?
The organization of elements in the periodic table makes is easier to identify the similarities and differences among different elements
98
What is similar about groups in the periodic table?
Elements in the same group in the periodic table generally have similar chemical properties

Chemistry Quiz 1 (4 decks)

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