BIG CHEM REVIEW Flashcards
(100 cards)
1
Q
very reactive, silver metals, can cut with butter knife, reacts with water to create a basic solution
A
alkali metals
2
Q
1st column on periodic table
A
alkali metals
3
Q
second column on periodic table
A
alkali earth metals
4
Q
reactive metals combined with non-metals in nature
A
alkali earth metals
5
Q
elements in groups 3-12
A
transition metals
6
Q
less reactive harder metals
A
transition metals
7
Q
wide range of physical and chemical properties
A
transition metals
8
Q
elements in group 17
A
halogens
9
Q
very reactive, volatile, diatomic, nonmetals
A
halogens
10
Q
most reactive nm
A
fluorine
11
Q
used as disinfectants and to strengthen teeth
A
fluorine
12
Q
elements in group 18
A
noble gases
13
Q
very unreactive/inert monatomic gases
A
noble gases
14
Q
have a full valence shell
A
noble gases
15
Q
properties of metals
A
shiny
silver
solid
good conductor
16
Q
nonmetals
A
dull
various colours
solid liquid and gas
poor conductors ]
17
Q
IUPAC
A
International Union of Pure and Applied Chemistry
18
Q
theoretical definition of elements
A
pure substances that are composed of only one kind of atom
19
Q
empirical definition of element
A
they cannot be broken down into simpler substances using chemical means such as heat or electricity
20
Q
elements that occur in more than one atom
A
h2 hydrogen,
I2 iodine
Cl2 chlorine
21
Q
elements on the left of the staircase line on the periodic table are classified as ______ and to the right are called _____
A
metals
non-metals
22
Q
What is chemisty?
A
the physical science that deals with composition properties and changes in matter
23
Q
define WHMIS
A
workplace hazardous materials information system
24
Q
changes in matter can be
A
physical changes
chemical changes
25
what is a physical change
no new substance is formed
26
what is chemical change?
at least one new substance is formed
27
define empirical knowledge
observable (from 5 senses)
can be qualitative or quantitative
28
define theoretical knowledge
explains the observables (ideas)
29
define mechanical separation
pick out parts of a mixture by hands or with a magnet
30
define settling separation
let components settle to the bottom of a container and then collect
31
define floatation separation
add chemicals to a mixture so that the desired components float and can be skimmed off
32
define filtration separation
pass heterogeneous mixture through a filter or a screen
33
define extraction seperation
combine a mixture with a solvent that dissolves the components
34
define distillation separation
boil a liquid to separate components based on boiling points
35
define crystallization separation
cool or concentrate a solution to get a dissolved solid
36
define chromatography separation
a mixture (pigment) is carried by a solvent through a porous material (filter paper) and different components are visible at different locations based on molecular size and mass
37
mechanical separation example
pick out parts of a mixture by hand or magnet
38
settling separation example
water treatment facility uses settling techniques
39
filtration separation example
furnace filter, vacuum filter, chemical filtration apparatus
40
distillation separation example
crude oil
41
ionic bond
the force that holds two opposite forces together
42
when atoms combine they form ions with the same electron arrangement as the nearest noble gas =
stable arrangement
full valence shell
43
four main types of ionic compounds
binary ionic compounds
44
define atoms
the smallest part of an element that still had properties of that element
45
atoms are made of sub-atomic particles
proton (p+)
electron (e-)
neutron (n0)
46
positive charge in nucleus
proton
47
negative charge, region surrounding nucleus
electron
48
no charge in nucleus
neutron
49
the atomic number tells the number of _____ in the nucleus atom
protons
50
the number of protons is equal to the number of
electrons
51
electrons orbit around in areas called
energy levels
52
electrons in the outermost energy level are known as
valence electrons
53
the # of valence electrons in an atom affects the way an atom will _____
bond
54
the way an _____ _____ determines many _______ of the
atom bonds
properties
element
55
groups of elements have similar bonding patterns and therefore
similar properties
56
if you looks at the atoms of every element in the vertical groups on the periodic table, you would notice that
each atom has the same number of valence electrons in its outermost shell
57
energy levels are the
PERIOD number
58
an ________ is about 2000x lighter than a ______ or ______
electron
proton
neutron
59
what are isotopes
atoms of the same element, they have the same number of protons but differ in neutron number
60
isotopes of the same element have identical
chemical properties
61
Isotopes have different
physical properties
62
atomic number =
number of protons
63
mass number =
number of protons + neutrons
64
formula for number of neutrons
mass number - atomic number = number of neutrons
65
draw an isotope format for aluminum and determine the number of neutrons for this isotope of aluminum
27 <---- mass number
Al
13 <---- atomic number
#n*= 27-13=14
66
when isotopes are radioactive they are called
radioisotopes
67
why would an element gain or lose an electron
to become stable (the octet rule)
68
How do you tell the difference between an atom and an ion
if there is a charge it is an ino
69
positively charged ions are called
cations
70
negatively charged ions are called
anions
71
Ions composed of only one type of atom
monatomic ions
72
A group of atoms with a net charge for the entire group
polyatomic ions
73
naming a cation
element name + ion
74
when do metals form cations?
when they lose electrons
75
naming anions
use a shortened element name with an "ide" ending + ion
76
non-metals form anions when they?
gain electrons
77
when atoms collide they may be a
transfer of electrons
78
when atoms collide they may be a
transfer of electrons
79
what happens to monatomic ions to achieve the most stable arrangement of electrons in each element
electrons transfer
80
positive ions will _______ electrons in the same amount as their _____
lose
charge
81
negative ions will _______ electrons in the same amount as their _____
gain
charge
82
ions will always have a
full valence shell (stable shell)
83
involves no change in formula or composition, BUT involves change in state and appearance
physical change
84
boiling water
physical change
85
involves a change in chemical bond
chemical change
86
which form of change requires more energy
chemical change requires more energy than physical change
87
cooking, combustion/burning
chemical change
88
one mole =
6.02 x 10^23
89
monatomic
means 1 - these elements exist alone
90
diatomic
means 2 - these elements have a buddy
91
polyatomic
exists as more than two - many of them together
92
memorized polatomics
P4(s) S8(s) O3(g)
93
memorized diatomics
H2(g) N2(g) O2(g) F2(g) Cl2(g) Br2(l) I2(s)
94
compounds made up of ONLY non-metal atoms are known as
molecular compounds
95
the bond between atoms are known as a
covalent bond
96
in molecular compounds, atoms ______ ______
share electrons
97
soluble in water (aqueous)
turns blue litmus red (ABR)
tastes sour (vinegar)
conducts electricity
corrodes metal (forms H2 bubbles)
properties of acids
98
usually written with hydrogen first (HCl)
can also appear with the "COOH" group at the end of the chemical formula
are usually written with the state aqueous
identifying acids
99
soluble in water
turns red litmus blue (BRB)
taste bitter (soap)
conducts electricity
no reaction with metal
slippery
properties of bases
100
written with an -OH group at the end of the chemical formula
are usually with the state aqueous
identifying bases
