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Spring 2014 > Chemistry Test 1 > Flashcards

Chemistry Test 1 Flashcards

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1
Q

Examples of Elemental Symbols

A

C, H, Be, S, Zn, etc

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2
Q

Examples of Compound Formula

A

CH4, H2O, CO, H2, SO4, etc

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3
Q

What is all matter composed of?

A

Atoms

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4
Q

An atom is composed of negatively charged particles called ________, that surround a positively charged nucleus

A

Electrons

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5
Q

What is the central core of an atom?

A

Nucleus

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6
Q

What does the nucleus consist of and what are they’re charges?

A

Protrons - positive

Neutrons - neutral

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7
Q

What is the atomic number?

A

The number of protrons (and electrons) in the nucleus.

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8
Q

What is the mass number?

A

The number of protrons plus the number of neutrons in the nucleus.

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9
Q

What are atoms with the same element that have different numbers of neutrons called?

A

Isotopes

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10
Q

What is an atomic mass unit (amu)?

A

1/12 the mass of a carbon-12 atom

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11
Q

What kind of force holds the nucleus together?

A

the strong force; the strongest force in the universe

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12
Q

What makes an atom radioactive?

A

When a nucleus emits particles from itself.

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13
Q

What is it called when a nucleus has more than 83 protrons, electric repulsions overcome the strong force, and the nucleus may spontaneously disintegrate?

A

Decay

the particles are emmtied from the nucleus to become more stable

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14
Q

What is a nuclei that undergoes spontaneous decay?

A

Radioactive isotope

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15
Q

The spontaneous process of uslei undergoin a change by emitting particles or rays is called

A

radioacitve decay or radioactivity

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16
Q

What are 3 common ways radioactive decay can occur?

A

alpha (), beta (ß), and gamma ()

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17
Q

The ability to break bonds in a molecule

A

Ionizing power

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18
Q

the measure of how far radiation can penetrate into a material and cause damage.

A

penetrating power

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19
Q

What is the radioactive decay equation?

A

A → B + b

A= parent nucleus

B= daughter nucleus

b= emitted particle ray

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20
Q

The disintegration of a nucleus with the emission of an alpha particle, equivalent to a helium nucleus is called

A

Alpha Decay

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21
Q

What is the ionizing power and penetrating power in alpha decay?

A

Ionizing Power - extremely high (massive in size (can’t go through people) and a charged (+2) particle); can attract e- from other molecules

Penetrating Power - weak (large in size)

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22
Q

What is the formula for alpha decay?

A

A → B + 42He

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23
Q

What is the disintegration of a nucleus by the emission of a beta particle (which is an electron) called?

A

Beta Particle

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24
Q

What is the formula for beta decay?

A

10n → 11p + 0-1e

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25
What is the ionizing power and the penetrating power of beta decay?
Ionizing - high (can go throught you) Penetrating - lower
26
What is it called when a nucleus emits a gamma ray and becomes a less energetic form of the same nucleus (usually from an excited state as a product of alpha or beta decay)?
Gamma Decay
27
What is the formula for a gamma decay?
\*A → B + g
28
the rate of decay of a given radionuclide, which is the time it takes for half of the nuclei in a sample to decay.
half-life
29
An easy way to remember half-life
1 = original sample 1/2 = 1st hl 1/4 = 2nd hl 1/8 = 3rd hl 1/16 = 4th hl 1/32 = 5th hl
30
What is the splitting of a large nucleus by bombarding it with neutrons to produce smaller nuclei, neutrons, and large amounts of energy called?
Fission
31
The release of neutrons bombard nearby nuclei and further fission occurs is called
Chain reaction
32
What is the minimum quantity of radioactive material called?
Critical mass (is needed to keep the reaction going)
33
What percentage of uranium is a fissionalbe 235U isotope?
0.7%
34
What are the rods made of in a nuclear reactor?
a neutron absorber ex - graphite
35
What are some advantages and disadvantages of nuclear power plants?
Advantages - 1.) to provide power to a city of 1,000,000 people requires 5,000,000 pounds of coal per day or 100 pounds of nuclear fuel; 2.) no production of green house gases Disadvantages - 1.) Security; 2.) disposal of waste; 3.) Improper control or removal of core generated heat can result in the fusing of "meltdown" of the fuel rods.
36
What is the process by which smaller nuclei combine to form larger ones, with the release of large amounts of energy called?
Fusion ex - stars
37
What is the difference between fission and fusion?
Fission - splitting a nucleus Fusion - fusing a nucleus together
38
Name the top 2 elemental compositions of the following: Earth's crust, Earth's core, the atmosphere, the human body, and the universe
Earth's crust - oxygen & silicon Earth's core - iron & nickel the atmosphere - nitrogen & oxygen the human body - oxygen & carbon the universe - hydrogen & helium
39
Name the classification of matter.
Matter = pure substances and mixtures Pure substances = elements and compounds Mixtures = heterogeneous mixture and homogeneous mixture
40
fixed compositions and identical properties; cannot be separated by physical means.
Pure substances
41
a substance in which all the atoms have the same number of protrons; give examples
element ex - F, Na, Cr
42
a substance composed of 2 or more elements chemically bonded in a fixed ratio; give examples
Compounds ex - NaCl, HF, H2O
43
composed of varying proportions of 2 or more substances that are just physically mixed, not chemically bonded; can be separated by physical means
mixture
44
nonuniform composition -- at lease 2 components; can be observed; give examples
heterogeneous mixture ex - italian dressing, concrete
45
looks uniform throughout -- appears as one substance give examples
homogeneous mixture ex - coffee, wine, gas, air, steel
46
an electrically neutral particle composed of 2 or more atoms chemically bonded; can be atoms of the same or different elements give examples
molecule ex - CO2, H2O, H2
47
Name the 7 diatomic molecules.
H2, N2, O2, F2, Cl2, Br2, I2 | (all are gases except Br2)
48
2 or more forms of the same element that have different bonding structures in the same physical state give examples
allotropes carbon has 3 allotropes - diamond, graphite, fullerenes oxygen has 2 allotropes - molecular oxygen (O2) and ozone (O3)
49
Name where the periods and groups are on the periodic table.
Periods - horizontal rows Groups - vertical rows
50
Name the 2 main groups of elements.
metals and non metals
51
Where are the metals, nonmetals, and metaloids/ semimetals located on the periodic table?
metals - to the left nonmetals - to the right semimetals - the shaded elements
52
tend to lose electrons in chemical reactions to form positive ions; good conductors;
metals
53
an atom or molecule that gained or lost electrons and forms a negative or positive charge
ion
54
Name and describe Group 1. Also name the ions it forms and how to write it.
Alkali Metals - highly reactive Ions - +1 how to write - Na+, K+, Be+
55
Name and describe Group 2. Also name the ion it forms and how to write it.
Alkaline Earth Metals - reactive Ions - +2 how to write - Na2+, Ca2+, Be2+
56
Name and describe Groups 3-12. Also name the ion it forms and how to write it.
Transition Metals - less reactive Ions - can form multiple ions; can form multiple charges how to write - b/c of multiple ions and charges, it can be writen multiple ways
57
What are Lanthanides?
Elements 58 - 70 on the periodic table; rare earth metals
58
What are Actinides?
elements 90 - 103 on the periodic table
59
elements whose atoms tend to gain (or share) electrons to form negative ions; poor conductors
nonmetals
60
Name and describe Group 17. Also name the ion it forms and how to write it.
Halogens - highly reactive Ions - -1 how to write - F-, Cl-, Br-, I-
61
Name and describe Group 18. Also name the ion it forms and how to write it.
Noble Gases - nonreactive; no charge; full electron orbitals (the "perfect" elements) Ions - no ions; no charge how to write - (Normal) He, Ne, Ar
62
Name and describe Group 16. Also name the ion it forms and how to write it.
No Name Given - Ions - -2 to the nonmetals only how to write - O2-, S2-
63
Name and describe Group15. Also name the ion it forms and how to write it.
No Name given - Ions - -3 to the nonmetals only how to write - N3-, P3-
64
Name and describe Group 13. Also name the ions it forms and how to write them.
No Name Given Ions - only B and Al are included; disregard the rest; +3 how to write - B3+, Al3+
65
electrons are found in various energy levels in atoms, called
shellls
66
How many electrons are in a shell?
8
67
What the outer shell of an atom called? What are the electrons in it called?
Valence shell; Valence electrons
68
For a given element what can the atomic number, period number and group number tell you?
Atomic number - number of electrons (and protrons) Period number - number of shells that contain electrons group number - Groups 1 and 2 - the number of valence electrons; Groups 13-18 - the number of valence electron = group number - 10
69
bonding by the attraction between oppositely charged ions; a transfer of electrons to form a full octet.
ionic bonding - has to be a metal and nonmetal
70
bonding by sharing one or more pairs of the same electrons.
covalent bonding - has to be 2 nonmetals
71
have both ionic and covalent characteristics; groups of covalently bonded atoms that have either lost or gained electrons
Polyatomic ions
72
Name the 7 polyatomic ions and their symbols.
ammonium ion - NH4+ cyanide ion - CN- hydroxide ion - OH- nitrate ion - NO3- sulfate ion - SO42- carbonate ion - CO32- phosphate ion - PO43-
73
How do you write Polyatomic Nomenclature?
Write the name of the first atom followed by the name of the polyatomic ion; if it has a positive charge it the polyatomic ion comes first, if it has a negative charge the polyatomic ion come last. Examples - HCN - Hydrogen Cyanide NaOH - Sodium Hydroxide K2Co3 - Potassium Carbonate Na2SO4 - Sodium Sulfate NaNO3 - Sodium Nitrate NH4Cl - Ammonium Chloride
74
How do you write the name of Ionic compounds?
The name of the first atom (metal) stays the same. The second (nonmetals) name changes to end in -ide. Examples- KCl - Potassium Chloride MgBr2 - Magnesium Bromide Li3N - Lithium Nitride BeCl2 - Beryllium Chloride MgS - Magnesium Sulfide
75
How do you write the name of a Covalent Compound?
Numerical prefixes are used to denote how many atoms of each element are in the compound; The name of the first element does not change, and if there is only one atom of the first element, no prefix is used; The second elements name (always has a prefix) changes to end in -ide. Examples- BF3 - Boron Trifluoide N2O - Dinitrogen Monooxide CO2 - Carbon Dioxode PCl5 - Phophorous Pentachloride N2O4 - Dinitrogen Tetroxide
76
What are the prefixes for naming covalent bonds?
1 - mono 5 - penta 2 - di 6 - hexa 3 - tri 7 - hepta 4 - tetra 8 - octa
77
metals that lose and electron to form a positive ion
cation
78
nonmetals gain an electron to form negative ions
anion

Spring 2014 (5 decks)

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