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chemistry 10 > BIG CHEM REVIEW > Flashcards

BIG CHEM REVIEW Flashcards

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1
Q

very reactive, silver metals, can cut with butter knife, reacts with water to create a basic solution

A

alkali metals

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2
Q

1st column on periodic table

A

alkali metals

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3
Q

second column on periodic table

A

alkali earth metals

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4
Q

reactive metals combined with non-metals in nature

A

alkali earth metals

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5
Q

elements in groups 3-12

A

transition metals

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6
Q

less reactive harder metals

A

transition metals

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7
Q

wide range of physical and chemical properties

A

transition metals

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8
Q

elements in group 17

A

halogens

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9
Q

very reactive, volatile, diatomic, nonmetals

A

halogens

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10
Q

most reactive nm

A

fluorine

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11
Q

used as disinfectants and to strengthen teeth

A

fluorine

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12
Q

elements in group 18

A

noble gases

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13
Q

very unreactive/inert monatomic gases

A

noble gases

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14
Q

have a full valence shell

A

noble gases

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15
Q

properties of metals

A

shiny
silver
solid
good conductor

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16
Q

nonmetals

A

dull
various colours
solid liquid and gas
poor conductors ]

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17
Q

IUPAC

A

International Union of Pure and Applied Chemistry

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18
Q

theoretical definition of elements

A

pure substances that are composed of only one kind of atom

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19
Q

empirical definition of element

A

they cannot be broken down into simpler substances using chemical means such as heat or electricity

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20
Q

elements that occur in more than one atom

A

h2 hydrogen,
I2 iodine
Cl2 chlorine

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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

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22
Q

What is chemisty?

A

the physical science that deals with composition properties and changes in matter

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23
Q

define WHMIS

A

workplace hazardous materials information system

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24
Q

changes in matter can be

A

physical changes
chemical changes

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25
Q

what is a physical change

A

no new substance is formed

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26
Q

what is chemical change?

A

at least one new substance is formed

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27
Q

define empirical knowledge

A

observable (from 5 senses)
can be qualitative or quantitative

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28
Q

define theoretical knowledge

A

explains the observables (ideas)

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29
Q

define mechanical separation

A

pick out parts of a mixture by hands or with a magnet

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30
Q

define settling separation

A

let components settle to the bottom of a container and then collect

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31
Q

define floatation separation

A

add chemicals to a mixture so that the desired components float and can be skimmed off

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32
Q

define filtration separation

A

pass heterogeneous mixture through a filter or a screen

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33
Q

define extraction seperation

A

combine a mixture with a solvent that dissolves the components

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34
Q

define distillation separation

A

boil a liquid to separate components based on boiling points

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35
Q

define crystallization separation

A

cool or concentrate a solution to get a dissolved solid

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36
Q

define chromatography separation

A

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

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37
Q

mechanical separation example

A

pick out parts of a mixture by hand or magnet

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38
Q

settling separation example

A

water treatment facility uses settling techniques

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39
Q

filtration separation example

A

furnace filter, vacuum filter, chemical filtration apparatus

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40
Q

distillation separation example

A

crude oil

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41
Q

ionic bond

A

the force that holds two opposite forces together

42
Q

when atoms combine they form ions with the same electron arrangement as the nearest noble gas =

A

stable arrangement
full valence shell

43
Q

four main types of ionic compounds

A

binary ionic compounds

44
Q

define atoms

A

the smallest part of an element that still had properties of that element

45
Q

atoms are made of sub-atomic particles

A

proton (p+)
electron (e-)
neutron (n0)

46
Q

positive charge in nucleus

A

proton

47
Q

negative charge, region surrounding nucleus

A

electron

48
Q

no charge in nucleus

A

neutron

49
Q

the atomic number tells the number of _____ in the nucleus atom

A

protons

50
Q

the number of protons is equal to the number of

A

electrons

51
Q

electrons orbit around in areas called

A

energy levels

52
Q

electrons in the outermost energy level are known as

A

valence electrons

53
Q

the # of valence electrons in an atom affects the way an atom will _____

A

bond

54
Q

the way an _____ _____ determines many _______ of the

A

atom bonds
properties
element

55
Q

groups of elements have similar bonding patterns and therefore

A

similar properties

56
Q

if you looks at the atoms of every element in the vertical groups on the periodic table, you would notice that

A

each atom has the same number of valence electrons in its outermost shell

57
Q

energy levels are the

A

PERIOD number

58
Q

an ________ is about 2000x lighter than a ______ or ______

A

electron
proton
neutron

59
Q

what are isotopes

A

atoms of the same element, they have the same number of protons but differ in neutron number

60
Q

isotopes of the same element have identical

A

chemical properties

61
Q

Isotopes have different

A

physical properties

62
Q

atomic number =

A

number of protons

63
Q

mass number =

A

number of protons + neutrons

64
Q

formula for number of neutrons

A

mass number - atomic number = number of neutrons

65
Q

draw an isotope format for aluminum and determine the number of neutrons for this isotope of aluminum

A

27 <—- mass number
Al
13 <—- atomic number
#n*= 27-13=14

66
Q

when isotopes are radioactive they are called

A

radioisotopes

67
Q

why would an element gain or lose an electron

A

to become stable (the octet rule)

68
Q

How do you tell the difference between an atom and an ion

A

if there is a charge it is an ino

69
Q

positively charged ions are called

A

cations

70
Q

negatively charged ions are called

A

anions

71
Q

Ions composed of only one type of atom

A

monatomic ions

72
Q

A group of atoms with a net charge for the entire group

A

polyatomic ions

73
Q

naming a cation

A

element name + ion

74
Q

when do metals form cations?

A

when they lose electrons

75
Q

naming anions

A

use a shortened element name with an “ide” ending + ion

76
Q

non-metals form anions when they?

A

gain electrons

77
Q

when atoms collide they may be a

A

transfer of electrons

78
Q

when atoms collide they may be a

A

transfer of electrons

79
Q

what happens to monatomic ions to achieve the most stable arrangement of electrons in each element

A

electrons transfer

80
Q

positive ions will _______ electrons in the same amount as their _____

A

lose
charge

81
Q

negative ions will _______ electrons in the same amount as their _____

A

gain
charge

82
Q

ions will always have a

A

full valence shell (stable shell)

83
Q

involves no change in formula or composition, BUT involves change in state and appearance

A

physical change

84
Q

boiling water

A

physical change

85
Q

involves a change in chemical bond

A

chemical change

86
Q

which form of change requires more energy

A

chemical change requires more energy than physical change

87
Q

cooking, combustion/burning

A

chemical change

88
Q

one mole =

A

6.02 x 10^23

89
Q

monatomic

A

means 1 - these elements exist alone

90
Q

diatomic

A

means 2 - these elements have a buddy

91
Q

polyatomic

A

exists as more than two - many of them together

92
Q

memorized polatomics

A

P4(s) S8(s) O3(g)

93
Q

memorized diatomics

A

H2(g) N2(g) O2(g) F2(g) Cl2(g) Br2(l) I2(s)

94
Q

compounds made up of ONLY non-metal atoms are known as

A

molecular compounds

95
Q

the bond between atoms are known as a

A

covalent bond

96
Q

in molecular compounds, atoms ______ ______

A

share electrons

97
Q

soluble in water (aqueous)
turns blue litmus red (ABR)
tastes sour (vinegar)
conducts electricity
corrodes metal (forms H2 bubbles)

A

properties of acids

98
Q

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

A

identifying acids

99
Q

soluble in water
turns red litmus blue (BRB)
taste bitter (soap)
conducts electricity
no reaction with metal
slippery

A

properties of bases

100
Q

written with an -OH group at the end of the chemical formula
are usually with the state aqueous

A

identifying bases

chemistry 10 (4 decks)

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