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Spring 2014 > Chemistry Test 1 > Flashcards

Chemistry Test 1 Flashcards

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
Q

What is the ionizing power and the penetrating power of beta decay?

A

Ionizing - high (can go throught you)

Penetrating - lower

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26
Q

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)?

A

Gamma Decay

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27
Q

What is the formula for a gamma decay?

A

*A → B + g

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28
Q

the rate of decay of a given radionuclide, which is the time it takes for half of the nuclei in a sample to decay.

A

half-life

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29
Q

An easy way to remember half-life

A

1 = original sample

1/2 = 1st hl

1/4 = 2nd hl

1/8 = 3rd hl

1/16 = 4th hl

1/32 = 5th hl

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30
Q

What is the splitting of a large nucleus by bombarding it with neutrons to produce smaller nuclei, neutrons, and large amounts of energy called?

A

Fission

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31
Q

The release of neutrons bombard nearby nuclei and further fission occurs is called

A

Chain reaction

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32
Q

What is the minimum quantity of radioactive material called?

A

Critical mass (is needed to keep the reaction going)

33
Q

What percentage of uranium is a fissionalbe 235U isotope?

A

0.7%

34
Q

What are the rods made of in a nuclear reactor?

A

a neutron absorber

ex - graphite

35
Q

What are some advantages and disadvantages of nuclear power plants?

A

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
Q

What is the process by which smaller nuclei combine to form larger ones, with the release of large amounts of energy called?

A

Fusion

ex - stars

37
Q

What is the difference between fission and fusion?

A

Fission - splitting a nucleus

Fusion - fusing a nucleus together

38
Q

Name the top 2 elemental compositions of the following:

Earth’s crust, Earth’s core, the atmosphere, the human body, and the universe

A

Earth’s crust - oxygen & silicon

Earth’s core - iron & nickel

the atmosphere - nitrogen & oxygen

the human body - oxygen & carbon

the universe - hydrogen & helium

39
Q

Name the classification of matter.

A

Matter = pure substances and mixtures

Pure substances = elements and compounds

Mixtures = heterogeneous mixture and homogeneous mixture

40
Q

fixed compositions and identical properties; cannot be separated by physical means.

A

Pure substances

41
Q

a substance in which all the atoms have the same number of protrons;

give examples

A

element

ex - F, Na, Cr

42
Q

a substance composed of 2 or more elements chemically bonded in a fixed ratio;

give examples

A

Compounds

ex - NaCl, HF, H2O

43
Q

composed of varying proportions of 2 or more substances that are just physically mixed, not chemically bonded; can be separated by physical means

A

mixture

44
Q

nonuniform composition – at lease 2 components; can be observed;

give examples

A

heterogeneous mixture

ex - italian dressing, concrete

45
Q

looks uniform throughout – appears as one substance

give examples

A

homogeneous mixture

ex - coffee, wine, gas, air, steel

46
Q

an electrically neutral particle composed of 2 or more atoms chemically bonded; can be atoms of the same or different elements

give examples

A

molecule

ex - CO2, H2O, H2

47
Q

Name the 7 diatomic molecules.

A

H2, N2, O2, F2, Cl2, Br2, I2

(all are gases except Br2)

48
Q

2 or more forms of the same element that have different bonding structures in the same physical state

give examples

A

allotropes

carbon has 3 allotropes - diamond, graphite, fullerenes

oxygen has 2 allotropes - molecular oxygen (O2) and ozone (O3)

49
Q

Name where the periods and groups are on the periodic table.

A

Periods - horizontal rows

Groups - vertical rows

50
Q

Name the 2 main groups of elements.

A

metals and non metals

51
Q

Where are the metals, nonmetals, and metaloids/ semimetals located on the periodic table?

A

metals - to the left

nonmetals - to the right

semimetals - the shaded elements

52
Q

tend to lose electrons in chemical reactions to form positive ions; good conductors;

A

metals

53
Q

an atom or molecule that gained or lost electrons and forms a negative or positive charge

A

ion

54
Q

Name and describe Group 1. Also name the ions it forms and how to write it.

A

Alkali Metals - highly reactive

Ions - +1

how to write - Na+, K+, Be+

55
Q

Name and describe Group 2. Also name the ion it forms and how to write it.

A

Alkaline Earth Metals - reactive

Ions - +2

how to write - Na2+, Ca2+, Be2+

56
Q

Name and describe Groups 3-12. Also name the ion it forms and how to write it.

A

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
Q

What are Lanthanides?

A

Elements 58 - 70 on the periodic table; rare earth metals

58
Q

What are Actinides?

A

elements 90 - 103 on the periodic table

59
Q

elements whose atoms tend to gain (or share) electrons to form negative ions; poor conductors

A

nonmetals

60
Q

Name and describe Group 17. Also name the ion it forms and how to write it.

A

Halogens - highly reactive

Ions - -1

how to write - F-, Cl-, Br-, I-

61
Q

Name and describe Group 18. Also name the ion it forms and how to write it.

A

Noble Gases - nonreactive; no charge; full electron orbitals (the “perfect” elements)

Ions - no ions; no charge

how to write - (Normal) He, Ne, Ar

62
Q

Name and describe Group 16. Also name the ion it forms and how to write it.

A

No Name Given -

Ions - -2 to the nonmetals only

how to write - O2-, S2-

63
Q

Name and describe Group15. Also name the ion it forms and how to write it.

A

No Name given -

Ions - -3 to the nonmetals only

how to write - N3-, P3-

64
Q

Name and describe Group 13. Also name the ions it forms and how to write them.

A

No Name Given

Ions - only B and Al are included; disregard the rest; +3

how to write - B3+, Al3+

65
Q

electrons are found in various energy levels in atoms, called

A

shellls

66
Q

How many electrons are in a shell?

A

8

67
Q

What the outer shell of an atom called?

What are the electrons in it called?

A

Valence shell; Valence electrons

68
Q

For a given element what can the atomic number, period number and group number tell you?

A

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
Q

bonding by the attraction between oppositely charged ions; a transfer of electrons to form a full octet.

A

ionic bonding - has to be a metal and nonmetal

70
Q

bonding by sharing one or more pairs of the same electrons.

A

covalent bonding - has to be 2 nonmetals

71
Q

have both ionic and covalent characteristics; groups of covalently bonded atoms that have either lost or gained electrons

A

Polyatomic ions

72
Q

Name the 7 polyatomic ions and their symbols.

A

ammonium ion - NH4+

cyanide ion - CN-

hydroxide ion - OH-

nitrate ion - NO3-

sulfate ion - SO42-

carbonate ion - CO32-

phosphate ion - PO43-

73
Q

How do you write Polyatomic Nomenclature?

A

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
Q

How do you write the name of Ionic compounds?

A

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
Q

How do you write the name of a Covalent Compound?

A

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
Q

What are the prefixes for naming covalent bonds?

A

1 - mono 5 - penta

2 - di 6 - hexa

3 - tri 7 - hepta

4 - tetra 8 - octa

77
Q

metals that lose and electron to form a positive ion

A

cation

78
Q

nonmetals gain an electron to form negative ions

A

anion

Spring 2014 (5 decks)

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