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Grade 10 > Chem > Flashcards

Chem Flashcards

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
Q

neutron

A

in nucleus, 1 amu, no charge, mass number-atomic number

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26
Q

electron

A

outside nucleus, 1/1887 amu, - charge, atomic number

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27
Q

Isotope is a

A

variation of an elemont with a different number of neutrons.

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28
Q

Isotopses are refered to by their

A

mass number

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29
Q

you can specity the isotope you are refrencing by using isotope notation. What is isotope notation

A

A (Mass number)
X (element symbol)
Z (Atomic Number)

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30
Q

Bohr rutherford is useful for predicting

A

the behaviour of atoms

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31
Q

Bohr rutherford neutrons and protons are in the, electrons

A

center of the diagram (nucleus) electrons are drawn in specific energy levels (shells, rings, orbitals)

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32
Q

Energy levels

A

2, 8, 8, 2, for the first energy level draw both electrons together

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33
Q

Gilbert lewis

A

covalent bond, dot structures, coined term “photon”

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34
Q

Lewis diagram shows

A

the chemical symbol and only the outermost valence energy level of electrons

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35
Q

Atoms are more stable when

A

they have a full valence shell

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36
Q

elements with fewer than 4 valence

A

metals, will lose electrons to create and full and stable shell

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37
Q

elements with more than 4 valence will

A

non-metals, gain electrons to create a full shell

38
Q

an atom has a positive charge if

A

it has lost an electron and has more protons than electrons

39
Q

an atom has a negative charge if

A

it has gained electrons, so it has more electrons than protons, thus it has a negative charge

40
Q

positive ion is called, negative ion is called

A

cation, anion

41
Q

elements in the same family (column)

A

devolp the same ionic charges

42
Q

metals tend to

A

lose electrons thus forming cations

43
Q

non-metals tend to

A

gain electrons, thus forming anions

44
Q

ions are

A

atoms that have lost or gained one or more elctrons resulting in a positive or negative charge.

45
Q

ionic compound is formed when

A

electrons are transfered creating positive or negative charges

46
Q

binary ionic compoud is

A

composed of a metal and a non-metal (cation and anion). The term binary indicates that ther are only 2 components

47
Q

naming binary ionic compounds

A

state the name of the metal, the the non metal changing the ending to ide

48
Q

writing chemical formulas for binary ionic compounds

A

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
Q

Some metals are able to form more than one ion we call these metals

A

multivalent meaning “multiple valence”, for example copper can form ions with a charge of +1 or +2, Cu+1 is pronounced copper one

50
Q

when you are refering to a multivalent metal you must

A

indicate which ion you are using in the name of the compound

51
Q

Ions formed from the attraction of several atoms are

A

covalent polyatomic, polyatomic means multipe atoms

52
Q

though polyatomic compounds are made of many atoms they

A

function as one specific ion

53
Q

a binary compound is composed of , a ternary compound is composed of

A

two, three

54
Q

polyatomic ions end with ? exceptions

A

ate, hydroxide, ammonium, cyanide

55
Q

naming polyatomic compounds

A

state the name of the cation (when multivalent indicate in roman numerals), state name of the anion

56
Q

writing formulas for polyatomic compounds

A

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
Q

Some elements are not strong enough to pull electrons away from other elements the elements

A

tend to share electrons in order to complete their outer shell

58
Q

molecular compounds are formed

A

when atoms of two or more different elements share electrons

59
Q

a covalent bond is formed

A

when electrons are shared between atoms

60
Q

binary molecular compounds are

A

compounds composed of two non-metals joined by one or more covalent bonds,

61
Q

naming covalent bonds

A

change the first non-metal to have the charge as if multivalent,

62
Q

prefixes 1,2,3,4,5

A

mono, di, tri, tetra, penta

63
Q

though we use the stock system you will see prefix system. give examples

A

carbon dioxide, carbon monoxide, carbon tetracloride, dinitrogen pentoxide

64
Q

what is a molecular formula

A

a chemical formula. It shows the number of atoms of each element.

65
Q

what is a structural formula

A

shows arrangement of atoms that make up a molecule

66
Q

diatomic elements

A

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
Q

which elements are diatomic

A

Hydrogen, Oxygen, Bromine, Florine, Iodine, Nitrogen, Chlorine

68
Q

As discrete elements not in compounds we wrute diatomic elements as

A

H2, O2, Br2, F2, I2, N2, CL2

69
Q

Diatomic elements are gases

A

at room temperature except for. Bromine which is a liquid and iodine which is solid

70
Q

Lewis Diagram - ionic

A

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
Q

Covalent Lewis Diagram

A

draw the lewis diagram for each, share electrons, simplify with lines

72
Q

in chemical reactions no

A

new mass is created, but rather atoms are rearranged to produce new combinations and thus new substancec

73
Q

word equationa and chemical equations

A

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
Q

Solid

A

state symbol s

75
Q

liquid

A

l

76
Q

gaseous

A

g

77
Q

aqueous

A

dissolved in water aq

78
Q

Antoine Lavoisier

A

discovery of oxygen in combustion, metric system, revised chemical nomenclature, law of convservation mass. “the father of modern chemistry”

79
Q

law of conservation mass

A

in a chemical reaction the total mass of the products will be the total mass of the reactants

80
Q

We need to balance the chemical equation by adding

A

coefficients in front of each chemical. we can’t change the formulas only the amount of each compound

81
Q

Ph paper

A

Acid-orange
neutral-yellow
base-blue

82
Q

blue litmus paper

A

acid-orange
neutral-same
base-blue

83
Q

red litmus paper

A

acid-same
neutral-same
base-blue

84
Q

HBB (bromothymol blue)

A

acid-yellow, neutral-green, base-dark blue

85
Q

Hpp (PHenolpthalein

A

acid-pale blue, neutral-mirky blue, base-dark purple

86
Q

Element

A

a pure substance that cannot be broken down further into a simpler substance. Made up of only one type of particle

87
Q

compound

A

a pure substance that can be broken down further into simpler substances. Made up of two or more elements

88
Q

period

A

a horizontal row of eleemtns (left to right) on the periodic table

89
Q

family, group

A

a vertical column of eleemtns up/down on the periodic table

90
Q
A

Grade 10 (6 decks)

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