Module 5 : Earth's Structure Flashcards

0
Q

(Matter Part 1 : Pure Substances and Mixtures)

List examples of pure substances and mixtures.

A
  • pure substance : gold (element), diamond (element), water (compound), methane (compound)
  • mixture : ocean water (salt, water, gases, etc.), rocks (different minerals), air (oxygen and water, other elements), not necessarily bonded together.
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1
Q

(Matter Part 1 : Pure Substances and Mixtures)

Describe the difference between a pure substance and a mixture

A
  • pure substance : an element or a compound; a substance with a fixed chemical composition
  • mixture : a combination of two or more pure substances
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2
Q

(Matter Part 1 : Pure Substances and Mixtures)

What is the difference between a heterogenous and homogenous mixture?

A
  • heterogenous mixture : a mixture in which the components are unevenly distributed
  • homogenous mixture : a mixture in which the components are evenly distributed
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3
Q

(Matter Part 1 : Pure Substances and Mixtures)

List examples of heterogenous and homogenous mixtures.

A
  • heterogenous mixture : citrus fruits, most rocks, mac and cheese
  • homogenous mixture : Alloy ring, ammonia mixture, air (local air)
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4
Q

(Matter Part 1 : Pure Substances and Mixtures)

What is a solution? Give examples.

A
  • a homogenous mixture in which one component is present in a much larger amount than the other component(s)
  • cup of tea, coffee, car cleaner, alloys, air
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5
Q

(Matter Part 1 : Pure Substances and Mixtures)
Identify each of the following as a pure substance or a mixture :
(A) oxygen gas
(B) ocean water
(C) blueberry muffin
(D) table salt

A

(A) oxygen gas : PURE SUBSTANCE
(B) ocean water : MIXTURE
(C) blueberry muffin : MIXTURE
(D) table salt : PURE SUBSTANCE

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6
Q

(Matter Part 1 : Pure Substances and Mixtures)
Identify each of the following as a homogenous or heterogenous mixture :
(A) sweetened tea
(B) fruit salad
(C) tap water
(D) noodle soup

A

(A) sweetened tea : HOMOGENOUS
(B) fruit salad : HETEROGENOUS
(C) tap water : HOMOGENOUS
(D) noodle soup : HETEROGENOUS

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7
Q
(Matter Part 1 : Pure Substances and Mixtures)
Which is an example of a pure substance?
(A) gasoline
(B) ocean water
(C) glucose
(D) air
A

ANSWER

(C) glucose

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8
Q
(Matter Part 1 : Pure Substances and Mixtures)
Which is an example of a solution?
(A) muddy water
(B) sports drink
(C) gelatin with fruit
(D) caramel popcorn
A

ANSWER

(B) sports drink

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9
Q

(Matter Part 2 : Phases of Matter)

Explain the differences between solids, liquids, and gases.

A
  • solid : a state of matter that has a definite shape and a definite volume.
  • liquid : a state of matter that has a definite volume, but no definite shape
  • gas : a state of matter that has neither a definite shape nor a definite volume
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10
Q

(Matter Part 2 : Phases of Matter)

Describe how adding heat to a substance affects the motion and arrangement of the particles

A
  • causes the molecules to move/vibrate quickly
  • further heating causes the particles in the liquid to move with such high amplitude vibrations that the attractions they have cannot hold them together
  • then they separate from one another forming gas
  • melting and evaporating can occur
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11
Q

(Matter Part 2 : Phases of Matter)

Describe how removing heat from a substance affects the motion and arrangement of the particles.

A
  • slower particles move, lower temperature, lower kinetic energy
  • eventually can freeze liquid
  • condensation and freezing can occur
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12
Q

(Matter Part 2 : Phases of Matter)
What happens to the arrangement of water molecules when it melts and freezes? How is this different that what would normally happen when a substance other than water gets colder and becomes a solid?

A
  • water (melts) : molecules begun to move around more and more and start to spread out, more dense
  • water (freeze) : molecules slow down and become more compacted, less dense
  • substance other than water (melts) : becomes less dense
  • substance other than water (freeze) : becomes more dense
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13
Q
(Matter Part 2 : Phases of Matter)
Which phases changes require an input of heat energy?
(A) melting and freezing
(B) melting and evaporation
(C) freezing and evaporation
(D) evaporation and condensation
A

ANSWER

(B) melting and evaporation

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14
Q

(Matter Part 2 : Phases of Matter)
Water freezing is different from most other liquids freezing because :
(A) water molecules break down when they freeze
(B) water freezes at a lower temperature than if melts
(C) water molecules are further apart in the solid than in the liquid
(D) water can freeze only if it is under high pressure

A

ANSWER

(C) water molecules are further apart in the solid than in the liquid

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15
Q
(Matter Part 2 : Phases of Matter)
To make tea, a person puts a pot of water on the stove. As the water absorbs the heat from the stove, what happens to the water molecules?
(A) They gain kinetic energy
(B) They bond tightly together
(C) They move more slowly
(D) They become less densely packed
A

ANSWER(S)
(A) They gain kinetic energy
(D) They become less densely packed

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16
Q

(Matter Part 3 : Atomic Structure)

What are elements?

A
  • substance up of only one kind of atom.
  • about 115 elements
  • examples : iron, gold, iodine, sulfur, lead
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17
Q

(Matter Part 3 : Atomic Structure)

What are nucleons?

A
  • a proton or neutron
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18
Q

(Matter Part 3 : Atomic Structure)

What is the difference between atomic number and mass number of an atom?

A
  • atomic number : the number of protons in an atom, determines element (kinda like a social security number)
  • mass number of an atom : the number of protons and neutrons in an atom, can vary from atom to atom
  • example an atom has 7 protons, 5 neutrons, and 7 electrons, what is the mass number? Answer = 12, specifically, nitrogen-12
    what is the atomic number = 7 which is Nitrogen on the periodic table
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19
Q

(Matter Part 3 : Atomic Structure)

atom

A
  • the smallest particle of an element

- building blocks of matter

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20
Q

(Matter Part 3 : Atomic Structure)

proton

A
  • located in the atomic nucleus
  • +1 charge, positively charged
  • large mass (1 amu)
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21
Q

(Matter Part 3 : Atomic Structure)

neutron

A
  • located in the atomic nucleus
  • no charge, electrically neutral
  • large mass (1 amu)
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22
Q

(Matter Part 3 : Atomic Structure)

electron

A
  • located outside of the atomic nucleus
  • -1 charge, negative charge
  • bound to electron cloud surrounding the outside of the nucleus
  • tiny mass (0 amu)
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23
Q

(Matter Part 3 : Atomic Structure)
An element’s atomic number is 14. What does this mean?
(A) Atoms of the element contain 14 neutrons.
(B) Atoms of the element contain 14 protons.
(C) Atoms of the element have a total of 14 protons and neutrons.
(D) Atoms of the element have a mass of 14 amu.

A

ANSWER

(B) Atoms of the element contain 14 protons

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24
Q

(Matter Part 3 : Atomic Structure)
Which atom has a mass number of 10?
(A) an atom with 14 protons and 4 neutrons
(B) an atom with 10 protons and 10 neutrons
(C) an atom with 6 protons and 4 neutrons
(D) an atom with 8 protons and 10 neutrons

A

ANSWER

(C) an atom with 6 protons and 4 neutrons

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25
Q

(Matter Part 3 : Atomic Structure)
Which atom has the greatest total mass?
(A) an atom with 5 protons and 4 neutrons
(B) an atom with 12 protons and 10 neutrons
(C) and atom with 8 protons and 8 neutrons
(D) an atom with 11 protons and 12 neutrons

A

ANSWER

(D) an atom with 11 protons and 12 neutrons

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26
Q

(Matter Part 4 : Electrons in Atoms)

How can you determine the overall charge of an atom if you know the number of protons and the number of electrons?

A
  • in a neutral atom, the number of protons equals the number of electrons
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27
Q

(Matter Part 4 : Electrons in Atoms)

In an electrically neutral atom, what must be true if the number of protons and electrons?

A
  • same number of protons and electrons

- +1 charges and -1 charges cancel each other out to create neutral

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28
Q

(Matter Part 4 : Electrons in Atoms)

Explain, using a diagram, the shell model of the atom.

A
  • SEE PAPER
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29
Q

(Matter Part 4 : Electrons in Atoms)

What are valance electrons? Label them in your diagram.

A
  • an electron in the outermost electron shell of an atom
  • determine properties of an element
  • stable valence electron is 8 valence electrons
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30
Q

(Matter Part 4 : Electrons in Atoms)
Which atom is electrically neutral?
(A) an atom with 14 protons and 4 electrons
(B) an atom with 10 protons and 10 electrons
(C) an atom with 4 protons and 8 electrons
(D) an atom with 10 protons and 11 electrons

A

ANSWER

(B) an atom with 10 protons and 10 electrons

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31
Q

(Matter Part 4 : Electrons in Atoms)
Which atom has a charge of +2?
(A) an atom with 12 protons and 10 electrons
(B) an atom with 10 protons and 12 electrons
(C) an atom with 12 protons and 12 electrons
(D) an atom with 2 protons and 2 electrons

A

ANSWER

(A) an atom with 12 protons and 10 electrons

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32
Q

(Matter Part 5 : Isotopes)

How are the three isotopes of hydrogen (H) (hydrogen-1, hydrogen-2, and hydrogen-3) different from one another?

A
  • hydrogen-1 : 1 proton, 0 neutron (protium)
  • hydrogen-2 : 1 proton, 1 neutron (deuterium)
  • hydrogen-3 : 1 proton, 2 neutrons (tritium)
  • all have the same atomic number
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33
Q

(Matter Part 5 : Isotopes)

How do the chemical and physical properties of isotopes of the same element compare?

A
  • chemical properties : same chemical properties
  • physical properties : same physical properties
  • same reactions
  • same compounds
  • same number of valence electrons
  • different mass number
  • may differ in radioactivity
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34
Q

(Matter Part 5 : Isotopes)

How can you determine the number of neutrons in an isotope if you know the atomic number?

A
  • subtract the atomic number from the mass number
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35
Q

(Matter Part 5 : Isotopes)

How does an atom of carbon-14 (14C) differ from an atom of carbon-12 (12C)?

A
  • carbon-14 has 8 neutrons

- carbon-12 has 6 neutrons

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36
Q

(Matter Part 5 : Isotopes)

isotope

A
  • atoms of an element that contain different numbers of neutrons
  • same atomic number, different mass numbers
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37
Q

(Matter Part 5 : Isotopes)
Chlorine (Cl) has two common isotopes, 35Cl and 37Cl. How are they different?
(A) They have different number of protons.
(B) They have different mass numbers.
(C) They react with different elements.
(D) They boil at different temperatures.

A

ANSWER

(B) They have different mass numbers.

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38
Q

(Matter Part 6 : Periodic Table)

Where on the periodic table are metals, nonmetals, and metalloids located?

A
  • metals : left and middle of the periodic table
  • nonmetals : top right corner of the periodic table
  • metalloids : diagonal in between the metals and nonmetals
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39
Q

(Matter Part 6 : Periodic Table)

What are general properties of metals, nonmetals, and metalloids?

A
  • metals : shiny, generally solid, good conductor, malleable and ductile
  • nonmetals : generally liquid or gas, poor conductor, brittle
  • metalloids : properties of metals and nonmetals
40
Q

(Matter Part 6 : Periodic Table)

Give some examples of how the properties of metals allow them to be used for a variety of purposes.

A
  • metals can be shaped and cut into sheets

- nonmetals include rust

41
Q

(Matter Part 6 : Periodic Table)

group

A
  • a column on the periodic table
42
Q

(Matter Part 6 : Periodic Table)

family

A
  • another term for a group
43
Q

(Matter Part 6 : Periodic Table)

period

A
  • a row on the periodic table
44
Q
(Matter Part 6 : Periodic Table)
Which group of elements has exactly two valence electrons?
(A) alkali metals
(B) alkaline earth metals
(C) halogens
(D) noble gases
A

ANSWER

(B) alkaline earth metals

45
Q
(Matter Part 6 : Periodic Table)
Which group of elements readily gain or share two valence electrons?
(A) alkali metals
(B) halogens
(C) chalcogens
(D) transition metals
A

ANSWER

(C) chalcogens

46
Q

(Matter Part 7 : Ionic Bonding)

What is the difference between an element and a compound?

A
  • element : a substance made up of only one atom, limited number of elements
  • compound : a substance made up of two or more elements that are chemically bonded together
47
Q

(Matter Part 7 : Ionic Bonding)

What is an ion?

A
  • a group of atoms with an overall electric charge
48
Q

(Matter Part 7 : Ionic Bonding)

When an electron loses an electron, what kind of ion does it become? What kind does it become when it gains an electron?

A
  • lose an electron : positive ion forms

- gain an electron : negative ion forms

49
Q

(Matter Part 7 : Ionic Bonding)

What happens to valance electrons when an ionic bond forms?

A
  • an atom that loses one or more valence electrons becomes positively charged, a positive ion
  • an atom that gains one or more valence electron becomes negatively charged, a negative ion
50
Q

(Matter Part 7 : Ionic Bonding)

What kinds of elements tend to lose electrons easily?

A
  • if an element is on the left side of the periodic table it will tend to lose because it’s easier to lose two electrons and have a full valence than it is to gain six electrons and have a full valence
  • sodium
51
Q

(Matter Part 7 : Ionic Bonding)

What kinds of elements tend to gain electrons easily?

A
  • if an element is on the right side of the periodic table, it will tend to gain electrons to have a valence of 8 electrons
  • fluorine
  • fluoride
52
Q

(Matter Part 7 : Ionic Bonding)

How can you use the periodic table to identify elements that will form an ionic bond with each other?

A
  • by looking at the number of valence electrons each atom has and how many each atom needs to complete its energy shell
53
Q

(Matter Part 7 : Ionic Bonding)

List examples of ionic compounds.

A
  • Sodium and chloride atoms = Sodium Chloride

- sodium and fluoride = Sodium Fluoride

54
Q

(Matter Part 7 : Ionic Bonding)

ionic bond

A
  • an electrostatic attraction between a positively charged ion and a negatively charged ion
55
Q
(Matter Part 7 : Ionic Bonding)
Elements in which group will form ionic bonds?
(A) group 1 and group 17
(B) group 17 and group 18 
(C) group 16 and group 17
(D) group 15 and group 17
A

ANSWER

(A) group 1 and group 17

56
Q
(Matter Part 7 : Ionic Bonding)
Which elements will form ionic bonds with the halogens?
(A) alkaline earth metals
(B) chalcogens
(C) noble gases
(D) other halogens
A

ANSWER

(A) alkaline earth metals

57
Q

(Matter Part 8 : Covalent Bonding)

What happens to valence electrons when a covalent bond forms?

A
  • atoms share valence electrons

- nonmetals tend to share valence electrons

58
Q

(Matter Part 8 : Covalent Bonding)

How can you use the periodic table to identify elements that will form covalent bonds with each other?

A
  • is formed when two atoms that tend to gain electrons are brought into contact with each other
  • atoms that tend to form covalent bonds are therefore primarily atoms of the nonmetallic elements in the upper right corner of periodic table (with the exception of the noble gas elements, which are very stable and tend not to form bonds at all)
59
Q

(Matter Part 8 : Covalent Bonding)

List examples of covalent compounds.

A
  • O3 : ozone
  • H2 : hydrogen
  • H2O : water
  • HCl : hydrogen chloride
  • CH4 : methane
  • NH3 : ammonia
  • CO2 : carbon dioxide
60
Q

(Matter Part 8 : Covalent Bonding)

covalent bond

A
  • a chemical bond resulting from the sharing of electrons between two atoms
61
Q
(Matter Part 8 : Covalent Bonding)
Elements in inch group will form covalent bonds?
(A) halogens
(B) transition metals
(C) alkali metals
(D) alkaline earth metals
A

ANSWER

(A) halogens

62
Q

(Matter Part 9 : Metallic Bonding)

What happens to valence electrons in a metallic bond?

A
  • electrons are able to move freely with other atoms, not just two atoms
  • aren’t fixed in certain positions
63
Q

(Matter Part 9 : Metallic Bonding)

How can you use periodic table to identify elements that will form metallic bonds with each other?

A
  • metallic binds will form with atoms of metal
64
Q

(Matter Part 9 : Metallic Bonding)

Explain why metals are conductors while nonmetals are insulators.

A
  • conductors (metals) : electric current can flow freely; outer electrons are loosely bound and free to move through material
  • insulators (nonmetals) : prevents flow of electrons; more stable atoms; outer electrons tightly bound
65
Q

(Matter Part 9 : Metallic Bonding)

malleable

A
  • able to be pounded into a thin sheet
66
Q

(Matter Part 9 : Metallic Bonding)

ductile

A
  • able to be pulled or stretched
67
Q

(Matter Part 9 : Metallic Bonding)

thermal conductor

A
  • a substance that transits heat easily
68
Q

(Matter Part 9 : Metallic Bonding)

electrical conductor

A
  • a substance that transmits electrical current easily
69
Q

(Matter Part 9 : Metallic Bonding)

metallic bond

A
  • a chemical bond in which metal atoms are joined together by freely flowing, loosely held electrons
70
Q

(Matter Part 9 : Metallic Bonding)
Why do nonmetals typically not conduct electricity well?
(A) They contain more protons than electrons.
(B) They can only gain valence electrons.
(C) Their valence electrons are tightly bound.
(D) Their protons are unable to leave the nucleus.

A

ANSWER

(C) Their valence electrons are tightly bound.

71
Q

(Earth’s Materials Part 1 : Rocks and Minerals)

What are minerals?

A
  • occur naturally
  • solid
  • mostly inorganic
  • fixed chemical formula
  • orderly crystalline structure
72
Q

(Earth’s Materials Part 1 : Rocks and Minerals)

What are some examples of silicate and nonsilicate minerals?

A
  • silicate minerals : make up most of the Earth’s crust, contain silicon and oxygen, rock forming material, easily form bonds, examples are Quartz, feldspar, and mica
  • nonsilicate minerals : contain no silicon, examples are gold, silver, diamond, table salt
73
Q

(Earth’s Materials Part 1 : Rocks and Minerals)

How are rocks related to minerals?

A
  • rocks are a combination of one or more minerals
74
Q
(Earth's Materials Part 1 : Rocks and Minerals)
Categorize each of the following rocks. Describe any unique characteristics of each rock : 
(A) granite
(B) conglomerate
(C) gneiss
(D) limestone
(E) dolomite
(F) basalt
A

(A) granite :
- usually 5 minerals
- usually light colored igneous rock that is found in continental crust
(B) conglomerate :
- sedimentary rock composed of rounded gravel-sized particles
(C) gneiss :
- metamorphic, foliated, medium to coarse grained texture, has light and dark bands, wide range of parent rocks
(D) limestone :
- usually 1 mineral
- sedimentary rock consisting mainly of calcium that was deposited by the remains of marine animals
(E) dolomite :
- sedimentary rock that consists of 50% calcium-magnesium carbonate; comes from mineral dolomite
(F) basalt :
- usually 3 minerals
- igneous volcanic rock that is composed of calcium-rich feldspar and other iron-rich minerals

75
Q

(Earth’s Materials Part 2 : Earth’s Layers)

What are the layers of the Earth?

A
  • crust
  • mantle
  • outer core
  • inner core
76
Q

(Earth’s Materials Part 2 : Earth’s Layers)

How are seismic P-waves different from seismic S-waves?

A
  • seismic P-waves : primary waves, longitudinal waves, travel through solid, liquid, gas, fastest waves
  • seismic S-waves : secondary waves, transverse waves, travel through solid only
77
Q

(Earth’s Materials Part 2 : Earth’s Layers)
How does the behavior of S-waves tell us that Earth’s mantle is solid? How does the behavior of S-waves tell us that Earth’s outer core is liquid?

A
  • seismic waves (S-waves) reflect from surfaces and refract through others
  • body waves travel through the Earth’s interior and can be called (P-waves or S-waves)
  • a scientist named Oldham inferred that how the P-waves traveled suggested the solid Earth becomes a liquid and he discovered that the Earth has a distinct core
  • body waves are used to determine the structure of the interior earth
78
Q

(Earth’s Materials Part 2 : Earth’s Layers)

Where does Earth’s magnetic field come from? Explain your answer in terms of the composition of the outer core.

A
  • the core generates magnetic field
  • liquid metal that makes up the outer core passes through a magnetic field, which causes an electric current, in turn, creates its own magnetic field that is stronger that the field that created it in the first place
79
Q

Quiz A

What statement correctly describes the chemical bond in sodium fluoride?

A
  • Sodium transfers an electron to fluorine, forming an ionic bond.
  • Ionic bonds form when electrons are transferred form one atom to another to gain stability. Cations, positively charged ions, result and are attracted by the electrical force forming an ionic bond.
80
Q

Quiz A

How does adding heat to ice affect the water molecules in the ice?

A
  • The added heat causes the molecules to vibrate more quickly.
  • Adding heat energy to a substance increases the kinetic energy of the molecules in the substance.
81
Q

Quiz A

What correctly describes the difference in the structure of carbon isotopes (C-12 and C-13)?

A
  • Carbon-12 has 6 neutrons and Carbon-13 has 7 neutrons.
  • Isotopes are very similar in their atomic structure having the same number of protons and electrons (including valence electrons). They differ because they have different numbers of neutrons which affects their atomic mass.
82
Q

Quiz A

How does the atomic structure of noble gases (He, Ne) differ from alkali metals (Na, K)?

A
  • Noble gases have full outer shells and alkali metals gain one.
  • Noble gases have full outer shells and do not react with other substances. Alkali metals have one valence electron in their outer shell and tend to form ionic bonds with halogens forming salts.
83
Q

Quiz A

What correctly describes the difference between a pure substance and a solution?

A
  • A salt crystal is a pure substance because it has a definite chemical composition and sugar water is a mixture because it does not.
  • Pure substances consist of one type of atom, molecule, or ion. Examples include hydrogen, helium, sodium chloride (salt), etc. Solutions are a type of mixture where the components are evenly distributed and finely mixed. Examples include sugar water and brass.
84
Q

Quiz A

Why does the silicate tetrahedron structural unit form many different kinds of silicate materials?

A
  • It can bond with oxygen atoms on other silicate tetrahedron and form chains, sheets, and three-dimensional networks.
  • The silicate tetrahedron structural unit forms many different minerals because of its ability to exist as single tetrahedra, chains, sheets, and three dimensional networks.
85
Q

Quiz A
A geologist discovers igneous rock layers in a particular area. What is the best conclusion for the geologist to form form this observation?

A
  • There was once a volcano in the area.

- Igneous rocks form when melted rock (magma or lava) cools and hardens. Magma and lava are commonly found at volcanoes.

86
Q

Quiz A

What correctly describes the conduction of heat?

A
  • Electrons in metals are loosely bound to their nuclei, allowing them to conduct heat easily.
  • Materials that are good conductors, like metals, contain metallic bonds which cause outer electrons to be weakly bonded to the nucleus. This allows electrons to move freely effectively conducting heat and electricity.
87
Q

Quiz A

How is the lithosphere different than the asthenosphere?

A
  • The lithosphere exhibits rigid behaviors and the asthenosphere acts in a plastic manner.
  • The lithosphere is the uppermost portion of the upper mantle. It is cooler than the asthenosphere and behaves in a rigid manner. The asthenosphere is below the lithosphere, is warmer, and flows slowly over time (plastic).
88
Q

Quiz A

What statement about the terms used to describe atoms is correct?

A
  • The atomic number indicates the number of protons contained in an atom of a specific element.
  • The atomic number is the number of protons in the nucleus of each element. The mass number is the total number of protons and neutrons in a specific isotope.
89
Q

Quiz B

What statement correctly describes covalent bonds?

A
  • Covalent bonds form between nonmetal atoms when the atoms share electrons.
  • Covalent bonds form when atoms share electrons. Two nonmetal atoms will form a covalent bond.
90
Q

Quiz B

What describes the molecular changes that occur when water condenses?

A
  • Decreased kinetic energy decreases the distance between molecules.
  • When the temperature drops, the kinetic energy of molecules decreases. As a result, molecules move slower and the space between them decreases.
91
Q

Quiz B
Sodium has an atomic number of 11 and a mass number of 23. It is in group 1 on the periodic table. How many valence electrons does it have?

A
  • 1
  • The number of valence electrons depends on the nu,her of electron shells. The first shell hold 2 electrons, the second shell holds 8, and the third shell holds 8. Since sodium has 11 electrons, it’s outer shell will have 1 electron.
92
Q

Quiz B

What two elements will form an ionic bond?

A
  • sodium (group 1) and bromine (group 17)
  • Sodium and bromine form ionic bonds when sodium donates an electron to bromine thus filling both atoms’ outermost shell.
93
Q

Quiz B

How are homogenous mixtures different than heterogenous mixtures?

A
  • Homogenous mixtures consist of two or more substances evenly mixed whereas the substances in heterogenous mixtures are not evenly mixed.
  • Homogenous mixtures exist when two or more substances are evenly mixed. Sugar water is homogenous because the sugar dissolves evenly in the water, unless the solution becomes supersaturated and the sugar materializes at the bottom. Heterogenous mixtures are not evenly distributed, like a piece of marble.
94
Q

Quiz B

What mineral is a nonsilicate?

A
  • halite (NaCl)

- Halite, or rock salt, is a nonsilicate mineral because it does not contain silicon (Si) and oxygen (O).

95
Q

Quiz B
What statement correctly describes the difference between a molecule of table salt (NaCl) and a molecule of methane (CH4)?

A
  • Sodium and chlorine form an ionic bond and carbon and hydrogen form covalent bonds.
  • The table salt molecule (NaCl) forms when sodium transfers an electron to chlorine forming an ionic bond with sodium and chloride ions arranged in a crystalline structure. Methane results when covalent bonds form between carbon and four hydrogen atoms and is found in natural gas.
96
Q

Quiz B

What affects the structure of igneous rock?

A
  • Chemical composition of parent magma and rate of cooling
  • Igneous rocks form when magma cools. The rate of cooling determines rock texture and the chemical composition of the parent magma determines rock color.
97
Q

Quiz B

What describes the properties of metamorphic rock?

A
  • Gneiss has a foliated texture due to compressional force.
  • Metamorphic rocks are formed when intense heat and pressure recrystallizes sedimentary and igneous rocks changing their mineral structure. Some metamorphic rocks have a foliated appearance when the pressure causes minerals to align in parallel bands.
98
Q

Quiz B

What statement correctly describes the Earth’s core?

A
  • It is responsible for Earth’s magnetic field.
  • The core is divided into inner and outer core. The inner core consists of iron and nickel in the solid state. The outer core is also composed of iron and nickel but the metals are in a liquid state which allows convection currents to create Earth’s magnetic field.