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Grade 10 > Chem > Flashcards

Chem Flashcards

(90 cards)

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1
Q

Synthesis

A

Making building
2 or more atoms compounds combine to form a new substance

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2
Q

Balancing equations

A

Remember only an arrow not an =
just make sure there are equal amounts on each side
atoms can leave compounds

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3
Q

Deomposition

A

Break down into two or more atoms

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4
Q

Single displacemnt

A

AKA sustitution reactions
a single element replaces another

A + BC - AC +B

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5
Q

Double displacement

A

Atoms in different compounds switch places to form two new compounds

AB + CD - AD +CB

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6
Q

Combustion

A

Burning of a hydrocarbon (compound containing only carbon and hydrogen atoms), in the prescence of oxygen

Hydrogen + oxygen - carbon dioxide + water

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7
Q

Incomplete combustion results in

A

Any combination of carbon containing compounds

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8
Q

Neutralization

A

Becomes water and ionic, acid and base cancel out each other. Special kind of double displacement, the hydrogen from the acid reacts with the hydroxide from the base to form H2O

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9
Q

Binary acids

A

Hydrogen and single non-metal

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10
Q

Oxyacid

A

Hydrogen and a polyatomic (oxy means oxygen)B

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11
Q

Bases

A

A molecule with a base of hydroxide or carbonate, or ammonia

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12
Q

Ph scale

A

How acidic or alkaline (basic)
goes from 0 to 14

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13
Q

Number alkali vs acid

A

0-6 acid
7 water
8-14 more alkaline

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14
Q

what does ph stand for

A

Power of hydrogen, concentrartion of Hydrogen

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15
Q

What is a base

A

pulls protons

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16
Q

What is an acid

A

Pulls electrons

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17
Q

Atomic Theory

A

All matter is made of atoms. Atoms of a pure substance are identical. Atoms can’t be created or destroyed. Atoms combine in simple ratios to form compounds

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18
Q

Who created atomic theory

A

democritus (400 BCE)
John Dalton 1807

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19
Q

JJ Thomson discovery in 1897

A

electrons

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20
Q

Marie Curie 1903

A

radiation

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21
Q

Ernest rutherford 1909, 1917

A

Atomic nucleus, protons

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22
Q

Niels Bohr 1913

A

electrons occupy discrete energy levels

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23
Q

James Chadwick 1932

A

neutrons

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24
Q

proton

A

in nucleus, 1amu, + charge, atomic number

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25
neutron
in nucleus, 1 amu, no charge, mass number-atomic number
26
electron
outside nucleus, 1/1887 amu, - charge, atomic number
27
Isotope is a
variation of an elemont with a different number of neutrons.
28
Isotopses are refered to by their
mass number
29
you can specity the isotope you are refrencing by using isotope notation. What is isotope notation
A (Mass number) X (element symbol) Z (Atomic Number)
30
Bohr rutherford is useful for predicting
the behaviour of atoms
31
Bohr rutherford neutrons and protons are in the, electrons
center of the diagram (nucleus) electrons are drawn in specific energy levels (shells, rings, orbitals)
32
Energy levels
2, 8, 8, 2, for the first energy level draw both electrons together
33
Gilbert lewis
covalent bond, dot structures, coined term "photon"
34
Lewis diagram shows
the chemical symbol and only the outermost valence energy level of electrons
35
Atoms are more stable when
they have a full valence shell
36
elements with fewer than 4 valence
metals, will lose electrons to create and full and stable shell
37
elements with more than 4 valence will
non-metals, gain electrons to create a full shell
38
an atom has a positive charge if
it has lost an electron and has more protons than electrons
39
an atom has a negative charge if
it has gained electrons, so it has more electrons than protons, thus it has a negative charge
40
positive ion is called, negative ion is called
cation, anion
41
elements in the same family (column)
devolp the same ionic charges
42
metals tend to
lose electrons thus forming cations
43
non-metals tend to
gain electrons, thus forming anions
44
ions are
atoms that have lost or gained one or more elctrons resulting in a positive or negative charge.
45
ionic compound is formed when
electrons are transfered creating positive or negative charges
46
binary ionic compoud is
composed of a metal and a non-metal (cation and anion). The term binary indicates that ther are only 2 components
47
naming binary ionic compounds
state the name of the metal, the the non metal changing the ending to ide
48
writing chemical formulas for binary ionic compounds
write symbols begining with metal, write ionic charge (no + or -), cross over the number writing in subscript (no subscript of 1), reduce to lowest terms
49
Some metals are able to form more than one ion we call these metals
multivalent meaning "multiple valence", for example copper can form ions with a charge of +1 or +2, Cu+1 is pronounced copper one
50
when you are refering to a multivalent metal you must
indicate which ion you are using in the name of the compound
51
Ions formed from the attraction of several atoms are
covalent polyatomic, polyatomic means multipe atoms
52
though polyatomic compounds are made of many atoms they
function as one specific ion
53
a binary compound is composed of , a ternary compound is composed of
two, three
54
polyatomic ions end with ? exceptions
ate, hydroxide, ammonium, cyanide
55
naming polyatomic compounds
state the name of the cation (when multivalent indicate in roman numerals), state name of the anion
56
writing formulas for polyatomic compounds
write symbols begininning with cation, write charges over each symbol, cros charges over, if polyatomic has charge greater than 1 put in brackets, reduce
57
Some elements are not strong enough to pull electrons away from other elements the elements
tend to share electrons in order to complete their outer shell
58
molecular compounds are formed
when atoms of two or more different elements share electrons
59
a covalent bond is formed
when electrons are shared between atoms
60
binary molecular compounds are
compounds composed of two non-metals joined by one or more covalent bonds,
61
naming covalent bonds
change the first non-metal to have the charge as if multivalent,
62
prefixes 1,2,3,4,5
mono, di, tri, tetra, penta
63
though we use the stock system you will see prefix system. give examples
carbon dioxide, carbon monoxide, carbon tetracloride, dinitrogen pentoxide
64
what is a molecular formula
a chemical formula. It shows the number of atoms of each element.
65
what is a structural formula
shows arrangement of atoms that make up a molecule
66
diatomic elements
in their natural state do not exist as individual atoms. Rather they exist naturally in pairs of atoms joined by one or more covalent bonds froming a molecule
67
which elements are diatomic
Hydrogen, Oxygen, Bromine, Florine, Iodine, Nitrogen, Chlorine
68
As discrete elements not in compounds we wrute diatomic elements as
H2, O2, Br2, F2, I2, N2, CL2
69
Diatomic elements are gases
at room temperature except for. Bromine which is a liquid and iodine which is solid
70
Lewis Diagram - ionic
Draw lewis for each element, draw arrow electron transfer, both ions must have full electron shells, finish by drawing brackets around the chemeical symbols with their valence shells and charges above
71
Covalent Lewis Diagram
draw the lewis diagram for each, share electrons, simplify with lines
72
in chemical reactions no
new mass is created, but rather atoms are rearranged to produce new combinations and thus new substancec
73
word equationa and chemical equations
chemists use equations to describe chemical reactions. Word equations show the names of each compounds and chemical equations show the formulas of the materials in the chemical. Reactants -> producst Starting substance turns to ending substance
74
Solid
state symbol s
75
liquid
l
76
gaseous
g
77
aqueous
dissolved in water aq
78
Antoine Lavoisier
discovery of oxygen in combustion, metric system, revised chemical nomenclature, law of convservation mass. "the father of modern chemistry"
79
law of conservation mass
in a chemical reaction the total mass of the products will be the total mass of the reactants
80
We need to balance the chemical equation by adding
coefficients in front of each chemical. we can't change the formulas only the amount of each compound
81
Ph paper
Acid-orange neutral-yellow base-blue
82
blue litmus paper
acid-orange neutral-same base-blue
83
red litmus paper
acid-same neutral-same base-blue
84
HBB (bromothymol blue)
acid-yellow, neutral-green, base-dark blue
85
Hpp (PHenolpthalein
acid-pale blue, neutral-mirky blue, base-dark purple
86
Element
a pure substance that cannot be broken down further into a simpler substance. Made up of only one type of particle
87
compound
a pure substance that can be broken down further into simpler substances. Made up of two or more elements
88
period
a horizontal row of eleemtns (left to right) on the periodic table
89
family, group
a vertical column of eleemtns up/down on the periodic table
90

Grade 10 (6 decks)

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