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Breaking Bad > Chapter 3 Test > Flashcards

Chapter 3 Test Flashcards

1
Q

What surrounds the nucleus in an atom

A

a cloudlike region of moving electrons

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2
Q

Where does most of the volume in an atom come from

A

the space in which electrons move

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3
Q

What is the symbol for an electron

A

e-

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4
Q

What is the charge of a neutron

A

0

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5
Q

How many electrons does it take to equal the mass of a proton

A

1,840

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6
Q

What unit is used to measure the mass of an atom

A

Atomic Mass Units

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7
Q

What is an atomic number

A

the number of protons in an element’s atom’s nucleus

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8
Q

What is a valence electron

A

the electrons in an atom with the highest amount of energy

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9
Q

Which atom is involved in chemical bonding

A

Valence electrons

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10
Q

What helps determine the chemical properties of an element

A

the number of valence electrons

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11
Q

What is the range of valence electrons an element can have

A

1 - 8

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12
Q

What is an electron dot diagram

A

a diagram of the symbol of the element and dots around it representing valence electrons

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13
Q

What element is stable with 2 val. electrons

A

Helium

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14
Q

What element only needs to gain 1 val. electrons to be stable

A

Hydrogen (keeps a stable 2)

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15
Q

What is a chemical bond

A

the force of attraction that holds atoms together as a result of the rearrangement of electrons between them

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16
Q

What group is the noble gasses

A

group 18 (Helium has 2 Val. electrons)

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17
Q

Do Noble Gasses react easily

A

no

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18
Q

How do metal atoms react

A

by losing their val. electrons

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19
Q

What group are Alkali metals in

A

group 1

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20
Q

What group are Halogens in

A

group 17

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21
Q

What does the reactivity of metal depend on

A

how easily its atoms lose val. electrons (the reactivity of metals reduces from left to right on the periodic table)

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22
Q

When Alkali metals (group 1) lose an electron they gain a stable arrangement of __ val. electrons

A

8

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23
Q

How reactive are Alkali metals

A

highly reactive

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24
Q

How do nonmetals become stable

A

they gain/share enough electrons to have 8 val. electrons (except the weirdo in the corner: Hydrogen who keeps a stable 2)

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25
Q

Can Halogens easily react with other elements

A

yes (they gain 1)

26
Q

Where are the metalloids on a periodic table

A

along the zigzag line

27
Q

how do metalloids combine with other elements

A

by losing or gaining electrons

28
Q

What is an ion

A

an atom/group of atoms with an electric charge

29
Q

When a neutral atom loses a valence electron it’s charge becomes ______

A

positive

30
Q

What is a polyatomic ion

A

an ion made of several elements

31
Q

What is an ionic bond

A

the attraction between 2 oppositely charged ions (metal <3 nonmetals)

32
Q

What is an ionic compound

A

the result of an ionic bond (a compound made of oppositely charged ions)

33
Q

What is a chemical formula

A

a group of symbols that shows the ratio of elements in a compound

34
Q

How is the name of an ionic compound writen

A

The name of the positive ion first then the negative one

35
Q

What does the suffix -ide mean in ionic compounds

A

that the negative ion is a single element

36
Q

What does the suffix -ate/-ite mean in ionic compounds

A

that the negative ion is polyatomic

37
Q

What crystals do ionic compounds form

A

hard, brittle crystals with high melting points which conduct electricity when dissolved in water or melted

38
Q

How do the ions in a compound need to be to conduct electricity

A

free moving

39
Q

What is a covalent bond

A

the bond between 2 atoms which share electrons

40
Q

What is a molecule

A

a neutral group of atoms joined by covalent bonds

41
Q

What is a double bond

A

When atoms share 2 pairs of electrons

42
Q

What is a triple bond

A

When atoms share 3 pairs of electrons

43
Q

What is a molecular compound

A

a compound made of molecules (covalently bonded)

44
Q

Which type of compound doesn’t conduct electricity and has a low melting point

A

molecular compound

45
Q

Why are molecular compounds poor conducters

A

because they don’t comtain charged particles

46
Q

Why do molecular compounds have a low melting point

A

because it’s bonds are weaker

47
Q

What does unequal sharing of electrons cause to covalently bonded atoms

A

it causes them to have slight electric charges

48
Q

What is a nonpolar bond

A

a covalent bond where electrons are shared equally

49
Q

What is a polar bond

A

a covalent bond where electrons are shared unequally (causes the atoms to have slight charges)

50
Q

What are van der Waals forces

A

The attractions in Polar molecules between slight negative and positive charges

51
Q

Which has stronger attraction? polar or nonpolar

A

polar

52
Q

Why do metal atoms easily lose electrons

A

because they do not hold onto them strongly

53
Q

What is a metal crystal composed of

A

closely packed, positively charged metal ions with valence electrons drifting among the ions

54
Q

What is a metallic bond

A

an attraction between a positive metal ion and the surrounding electrons

55
Q

What are the properties of metals

A

shiny luster and high levels of malleability, ductility, thermal and electrical conductivity

56
Q

Why does metal have a shiny and reflective luster

A

because the valence electrons absorb and remit light

57
Q

What does it mean if something is ductile

A

it can easily be dent and pulled into wire

58
Q

What does it mean if something is malleable

A

it can be rolled into (thin) sheets and hammered into shape

59
Q

Why are metals ductile and malleable

A

because positive metal ions are attracted to the loose electrons around them rather than to other metal ions

60
Q

Why do metals have high thermal and electrical conductivity

A

because the electrons are free to move

61
Q

What is an alloy

A

a mixture of 2 or more elements of at least one is metal

Breaking Bad (8 decks)

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