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AP Chemistry > Textbook Ch.2: Atoms, Molecules, and Ions > Flashcards

Textbook Ch.2: Atoms, Molecules, and Ions Flashcards

1
Q

What are the three parts of Dalton’s atomic theory?

A
  1. An element is composed of tiny particles called atoms. All atoms of a given element show the same chemical properties. Atoms of different elements show different properties
  2. In an ordinary chemical reaction, atoms move from one substance to another, but no atom of any element disappears or is changed into an
    atom of another element
  3. Compounds are formed when atoms of two or more elements combine. In a given compound, the relative numbers of atoms of each kind are definite and constant. In general, these relative numbers can be expressed as integers or simple fractions
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2
Q

Atom

A

the smallest particle of an element that can enter into a chemical reaction

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3
Q

Electrons

A

negatively charged particles that are common to all atoms, and carry a unit negative charge (-1), and have a very small mass, roughly 1/2000 that of the lightest atom

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4
Q

Protons

A

has a mass nearly equal to that of an ordinary hydrogen atom. The proton carries a unit positive charge (+1), equal in
magnitude to that of the electron (-1)

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5
Q

Neutrons

A

uncharged particles with a mass slightly greater than that of a proton

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6
Q

Law of conservation of mass

A

there is no detectable change in mass in an ordinary chemical reaction. If atoms are conserved in a reaction, the atomic mass will also be conserved

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7
Q

Law of constant composition

A

a compound always contains the same elements in the same proportions by mass. If the atom ratio of the elements in a compound is fixed, their proportions by mass must also be fixed

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8
Q

Law of multiple proportions

A

Applies in situations in which two elements form more than one compound

The law states that in these compounds, the masses of one element that combine with a fixed mass of the second element are in a ratio of small whole numbers

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9
Q

Atomic number

A
  • All the atoms of a particular element have the same number of protons in the nucleus
  • Given the symbol Z
    Z = number of protons
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10
Q

In a neutral atom…

A

the number of protons = number of electrons

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11
Q

Mass number

A
  • Found by adding up the number of protons and neutrons in the nucleus
  • Given the symbol A
    A = number of protons + number of neutrons
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12
Q

All atoms of a given element have the same _____, however, they can differ from one another in _____

A

all atoms of a given element have the same atomic number (Z), but they differ from one another in mass number (A)

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13
Q

Isotopes

A

atoms that contain the same number of protons but a different number of neutrons

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14
Q

Nuclear symbol

A

A symbol that shows the composition of a nucleus

  • The atomic number (Z) appears as a subscript on the lower left of the symbol of the element
  • The mass number (A) is written as a superscript in the the upper left
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15
Q

Radioactivity

A

when unstable isotopes decompose (decay)

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16
Q

Transmutation of elements

A
  • The result of radioactivity
  • The atomic number of the product nucleus differs from that of the reactant
  • Can be beta particles identical in their properties to electrons
  • Can be alpha particles, which are The particles Z=2, A=4 carrying a +2 charge
  • Can be gamma rays, which consist of high-energy radiation
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17
Q

Periodic table

A

an arrangement of elements, in order of increasing atomic number, in horizontal rows of such a length that elements with similar chemical properties fall directly beneath one another in vertical groups

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18
Q

Periods

A

the horizontal rows in the periodic table

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19
Q

Groups

A

the vertical columns in the periodic table

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20
Q

Main-group elements

A

elements falling in Groups 1,2,13,14,15,16,17, and 18

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21
Q

Transition metals

A

elements falling in Groups 3-12

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22
Q

Post-transition metals

A

the metals in groups 13, 14, and 15

23
Q

Alkali metals

A

a special name for the elements in group 1

  • Lithium (Li), sodium (Na), and potassium (K) in this group all react vigorously with water to produce hydrogen gas
24
Q

Alkaline earth metals

A

a special name for the elements in group 2

25
Q

Halogens

A

a special name for the elements in group 17

26
Q

Noble gases

A

a special name for the unreactive gases in group 18

  • Helium (He), neon (Ne), and argon (Ar) do not react with any other substance
27
Q

A diagonal line or stairway that starts to the left of boron in the periodic table separates ____ from ____

A

separates metals from nonmetals

28
Q

Metals

A

elements with high electrical conductivities

29
Q

Nonmetals

A

elements with low electrical conductivities

30
Q

Metalloids

A
  • Elements that are difficult to classify exclusively as metals or nonmetals
  • They have properties between those of elements in the two classes
  • Their electrical conductivities are intermediate between those of metals and nonmetals
  • Boron (B), silicon (Si), germanium (Ge), arsenic (As), antimony (Sb), and tellurium (Te)
31
Q

Ions

A

formed when an atom loses or gains electrons

32
Q

Cations

A

positively charged ions

33
Q

Anions

A

negatively charged ions

34
Q

What happens to the subatomic particles of an atom when an ion is formed?

A
  • The number of protons in the nucleus is unchanged

- The number of electrons increases or decreases

35
Q

Monatomic ions

A

ions derived from a single atom by the loss or gain of electrons

36
Q

Polyatomic ions

A

ions containing more than one atom

  • the atoms are held together by covalent bonds in polyatomic ions
  • you can think of polyatomic ions as a “charged molecule”
37
Q

Ionic compounds

A

Compounds that contain both cations and anions in order to be electrically neutral

  • Held together by STRONG electrical forces between oppositely charged ions referred to as ionic bonds
38
Q

What are some properties of ionic compounds?

A
  • Solids at room temperature
  • Have relatively high melting points
  • To melt an ionic compound requires that oppositely charged ions be separated from one another, thereby breaking ionic
    bonds
39
Q

Strong electrolyte

A

made when an ionic solid dissolves in water and therefore causing the ions to separate and the solution to conduct an electric current

40
Q

Non-electrolytes

A

made when a molecular solid dissolves in water and does not conduct electricity

41
Q

What does the principle of electrical neutrality require?

A

the total positive charge of the cations in the formula must be equal to the total negative charge of the anions

42
Q

How can the charges of ions formed by atoms of the main-group elements be predicted?

A

atoms that are close to a noble gas (Group 18) in the periodic table form ions that contain the same number of electrons as the neighboring noble-gas atom

43
Q

How are monatomic cations of main-group elements named?

A

take the name of the metal from which they are derived

Na+ sodium
K+ potassium

44
Q

How are monatomic cations of transition and post-transition elements named?

A

with a roman numeral representing the charge because they can have multiple charges

Fe2+ iron (II)
Fe3+ iron (III)

45
Q

How are monatomic anions named?

A

by adding the suffix -ide to the stem name of the nonmetal from which they are derived

46
Q

Oxoanion

A

certain non-metals in Groups 15-17 of the periodic table form more than one polyatomic ion containing oxygen

47
Q

How is the polyatomic ion named when a nonmetal forms two oxoanions?

A
  • the suffix -ate is used for the anion with the largest number of oxygen atoms
  • the suffix -ide is used for the anion containing fewer oxygen atoms
48
Q

How is the polyatomic ion named when a nonmetal forms more than two oxoanions?

A
  • The prefix per- is used meaning the largest number of oxygen atoms
  • The prefix hypo- is used meaning the fewest oxygen atoms
49
Q

What are the two words in an ionic compound?

A
  • The first word names the cation

- The second word names the anion

50
Q

Binary molecular compounds

A

when two nonmetals combine with each other

51
Q

Describe the systematic way of naming a binary molecular compound.

A
  • The first word gives the name of the element that appears first in the formula
  • A Greek prefix is used to show the number of atoms of that element in the formula
  • The second word consists of the appropriate Greek prefix designating the number of atoms in the second element
52
Q

Acids

A

when a few binary molecular compounds containing H atoms ionize in water to form H⁺ ions

53
Q

Oxoacids

A

acids that contain oxygen in addition to hydrogen

54
Q

How are the prefixes replaced when dealing with oxoacids?

A
  • -ate is replaced by -ic

- - ite is replaced by -ous

AP Chemistry (11 decks)

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