Unit 1: Atomic Structure & Property

Question 1

Homogenous mixture (solution)

Answer 1

The
composition of the mixture is the same
throughout (at the atomic/molecular level).

Question 2

Heterogeneous mixture

Answer 2

The composition is
not uniform throughout.

Question 3

compound (chemical means)

Answer 3

a substance composed of atoms
of two or more elements chemically united in fixed
proportions

Question 4

extensive property

Answer 4

depends upon
how much matter is is being considered

Question 5

intensive property

Answer 5

does not
depend upon how much matter is is being
considered

Question 6

density=

Answer 6

m/V

Question 7

Avogadro’s number (number of atoms in 12 g of carbon-12)

Answer 7

6.022 x 10(^23)

Question 8

Sig Figs

Answer 8

-significant= not zero, sandwich zeros, right of decimal point
-not significant= left of first nonzero digit
-addition- smallest decimal

Question 9

Isotopes

Answer 9

are atoms of the same element (same number of
protons) but different numbers of neutrons in their nuclei.

Question 10

molecule

Answer 10

an aggregate of two or more atoms in a definite arrangement held together by covalent bonds.

Question 11

ion

Answer 11

atom, or group of atoms, that has a net
positive or negative charge (cations lose, anions gain)

Question 12

Dalton’s Laws

Answer 12

-Multiple proportions (ratio of compound)
-Conservation of Mass

Question 13

molecular formula

Answer 13

exact number of
atoms of each element in a molecule of the
substance.

Question 14

empirical formula

Answer 14

simplest
whole-number ratio of the atoms in a substance.

Question 15

ionic compounds

Answer 15

combination of cations
and anions, formula is always the same as the empirical formula, sum of the charges on the cation(s) and anion(s) in each formula unit must equal zero

Question 16

Montamic anion names end in

Answer 16

ide (ex. nitride) (so ionic compound would be metal+nonmetal, barium chloride)

Question 17

Transition metal ionic compounds

Answer 17

ex. iron (II) chloride
-ic, refer to a cation with a larger charge.
-ous, suffix indicates the cation with the lesser relative cation charge,

Question 18

Molecular compounds

Answer 18

-Made of nonmetals or nonmetals +
metalloids
-element further left and bottom n periodic table is first.
-prefix mono, di, etc then last ends in “ide”

Question 19

acid

Answer 19

-yields hydrogen ions (H+) when dissolved in water
-ex. HCl
-(oxoacid contained H, O, and another element)

Question 20

base

Answer 20

-substance that yields
hydroxide ions (OH–) when dissolved in water
-ex. NaOH

Question 21

Hydrates

Answer 21

-compounds that have a specific
number of water molecules attached to them.
-

Question 22

Functional Group

Answer 22

in orgo chem, specific group of atoms or bonds within a compound that is responsible for the characteristic chemical reactions of that compoundd

Question 23

For any element
atomic mass (amu) =

Answer 23

molar mass (grams)

Question 24

Molecular mass

Answer 24

the sum of
the atomic masses (in amu) in a molecule

Question 25

Formula mass

Answer 25

sum of the atomic masses
(in amu) in a formula unit of an ionic compound

Question 26

Percent Composition and Empirical Formulas

Answer 26

assume 100g
%–>assume g–>mol (divide by smallest)

Question 27

Limiting Reactants

Answer 27

1. balance 2. grams given–> moles 3. moles of the desired product (based on _) using mole ratio 4. keep the smaller number

Question 28

Electromagnetic
radiation

Answer 28

the emission
and transmission of energy
in the form of
electromagnetic waves

Question 29

speed of light=

Answer 29

wavelength (lambda) times frequency

Question 30

Energy(discrete units, quantum)=

Answer 30

h(plank’s constant) x v

Question 31

1st Ionization energy

Answer 31

-the strength of the coulombic attraction of the outermost, easiest to remove, electron to the nucleus
-increases across period (as #protons increase in same energy level)
-decreases down group as e- in higher energy level (shielding)

Question 32

ionization chart

Answer 32

Large jump in IE when removing less-shielded core electrons (2nd & subsequent IE’s increase as coulombic attraction of remaining e–’s to nucleus increases)

Question 33

Aufbau principle

Answer 33

Fill up” electrons in lowest energy orbitals

Question 34

Hund’s rule

Answer 34

The most stable arrangement of electrons in subshells is the one with the greatest number of parallel spins

Question 35

orbitals

Answer 35

s (1), p (3), d (5), f (7)

Question 36

Effective nuclear charge (Zeff)

Answer 36

the “positive charge” felt
by an electron

Question 37

Is cation or anion smaller than atom form?

Answer 37

-Cation is always smaller than atom from which it is formed.
-Anion is always larger than atom from which it is formed.

Question 38

Electron affinity

Answer 38

the negative of the energy change that occurs when an electron is accepted by an atom in the gaseous state to form an anion.

Question 39

solution

Answer 39

homogenous mixture of 2 or more
substances

Question 40

solute

Answer 40

substance(s) present in the
smaller amount(s)

Question 41

solvent

Answer 41

substance present in the larger
amount

Question 42

electrolyte

Answer 42

when dissolved in
water, results in a solution that can conduct electricity.

Question 43

nonelectrolyte

Answer 43

substance that, when dissolved,
results in a solution that does not conduct electricity (free moving pathway for electrons)

Question 44

Weak Electrolyte – not completely dissociated

Answer 44

–> over <—

Question 45

Strong Electrolyte

Answer 45

100% dissociation

Question 46

Always soluble- solubility rules

Answer 46

N (nitrates No3-)
A (acetates C2H3O2-)
G (group 1)

S (sulfates SO4-2)
A (ammonium NH4+)
G (group 17)

Question 47

Exceptions

Answer 47

—(to sulfates and group 17)
P (lead Pb+2)
M (Mercury Hg2+2)
S (silver Ag+)

—(to sulfates)
Castro Bear
Ca+2
Sr+2
Ba+2