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1
Q

matter

A

anything that takes up space and has mass

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2
Q

chemistry

A

the study of matter

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3
Q

physical properties

A

characteristics that can be observed or measured without changing chemical identity (colour, texture)

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4
Q

chemical properties

A

describe the ability of matter to react with another substance to form different substances (combustibility, lack or reactivity)

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5
Q

physical change

A

change of matter that does not alter its chemical identity or composition (freezing of water to form ice)

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6
Q

chemical change

A

change of matter that produces new substances (colour change, formation of bubbles)

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7
Q

atoms bond together to form…

A

ionic and covalent compounds

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8
Q

can mass be created or destroyed in chemical reaction

A

no

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9
Q

a chemical equation represents…

A

what happens to atoms in a reaction

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10
Q

pure substance

A

can be element or compound

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11
Q

compound

A

made up of atoms of 2 or more different elements

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12
Q

ionic compound

A

compound made up of oppositely charged ions. consists of positively charged ions, cations, and negatively charged ions, called anions.

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13
Q

ionic bond

A

strong attraction that forms between oppositely charged ions. in this, atoms lose or gain electrons to form ions that have full valence shells and are therefore more stable

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14
Q

covalent compound

A

compound that results when 2 or more atoms of non metal elements bond covalently

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15
Q

covalent bond

A

strong attraction between atoms that forms when atoms share valence electrons

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16
Q

molecule

A

particle made up of two or more atoms bonded by covalent bonds. most covalent compounds exist as molecules

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17
Q

elements combine with compounds to form…

A

new compounds and new elements

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18
Q

energy is required to ___ chemical bonds

A

break

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19
Q

energy is ___ when chemical bonds form

A

released

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20
Q

closed system

A

energy can enter or leave but not matter

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21
Q

open system

A

energy and matter can enter or leave

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22
Q

law of conservation of mass

A

in a chemical reaction, the total mass of the substances used is equal to the total mass of the substances produced

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23
Q

chemical equation

A

the representation of a chemical reaction using words or chemical formulas

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24
Q

reactant

A

a substance that undergoes a chemical change

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25
Q

product

A

a substance formed in a chemical change

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26
Q

word equation

A

shows the names of the chemical elements and compounds in a chemical reaction

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27
Q

skeleton equation

A

shows the chemical formulas in a chemical reaction

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28
Q

balanced equation

A

shows the reactants and products in the chemical equation with coefficients

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29
Q

diatomic elements

A

two of the same elements joined by a covalent bond (H2, N2, O2, F2, Cl2, Br2, I2)

30
Q

polyatomic elements

A

many atoms of the same element joined by a covalent bond (S8, P4)

31
Q

subscripts

A

indicate how many atoms of each element are present (in Al2Br3, 2 and 3 are the subscripts)

32
Q

coefficients

A

indicate how many molecules are present (in 2S8, 2 is the coefficient)

33
Q

how do u balance a chemical equation

A

number of atoms on the reactant side must equal number of atoms on product side. law of conservation of mass is reflected in balanced chemical equation. use coefficients in front of chemical formula

34
Q

matter and energy react in __ and __ changes

A

physical and chemical

35
Q

there is a transfer of energy between chemical reactions and the…

A

surroundings

36
Q

energy

A

needed for everyday processes, transferred between system and surroundings. energy that leaves system enters surroundings, energy that enters system came from surroundings

37
Q

activation energy

A

minimum amount of energy needed for reaction to happen

38
Q

in chemical reactions, reactants must…

A

collide with enough energy to break bonds

39
Q

energy changes occur with all…

A

chemical reactions

40
Q

photosynthesis

A

process that captures sunlight to produce sugar molecules for plants

41
Q

animals that eat plants can use energy stored in sugar through…

A

cellular respiration

42
Q

exothermic reaction

A

chemical reaction in which there is net release of energy to surroundings. temperature increases as energy is released into surroundings

43
Q

endothermic reaction

A

chemical reaction in which there is net absorption of energy from the surroundings. temperature decreases as energy is absorbed by system

44
Q

cellular respiration equation

A

C6H12O6 + 6O2 = 6CO2 + 6H2O

45
Q

energy-level diagrams

A

show energy changes in a reaction. in endothermic reaction, energy of product is greater than that of reactants. in exothermic reaction, energy of product is less that that of reactants.

46
Q

synthesis reaction

A

chemical reaction in which 2 or more reactants combine to form single product. most are exothermic. A + B = AB

47
Q

decomposition reaction

A

chemical reaction in which compound is broken down into elements or simpler compounds. most are endothermic. AB = A + B

48
Q

single replacement reaction

A

chemical reaction in which an element and compound react to produce another element and another compound. A + BX = AX + B

49
Q

double replacement reaction

A

chemical reaction in which solutions of 2 ionic compounds react to produce 2 new compounds. precipitate (ppt) is usually produced. metal replaces metal, non metal replaces non metal. AX + BY = AY + BX

50
Q

combustion reaction

A

chemical reaction in which compound or element reacts with oxygen to produce an oxide of element. many produce heat and light. also refers to burning of hydrocarbons to produce CO2 and H2O

51
Q

hydrocarbon

A

compound that consists of carbon and hydrogen. general equation for combustion of hydrocarbon is CxHy + O2 = CO2 + H2O. hydrocarbon combustions are exothermic.

52
Q

incomplete combustion

A

occurs when low amounts of oxygen are available. produces carbon dioxide, water, carbon monoxide and soot

53
Q

acid

A

compound that forms H+ ions when dissolved in water. chemical formula for acid has H in it

54
Q

binary acid

A

consists of hydrogen and non-metal (HCl)

55
Q

oxyacid

A

consists of hydrogen, oxygen and another element (H2CO3)

56
Q

base

A

compound that forms OH- ions when dissolved in water. chemical formula for base has OH in it

57
Q

acid-base indicators

A

used to identify acids and bases by changing colours

58
Q

pH scale

A

used to measure pH. ranges from 0-14, if solution has pH if less than 7, it’s acidic. basic solutions have pH of greater than 7. neutral substances have pH of equal to 7.

59
Q

neutralization reaction

A

chemical reaction in which acid reacts with base to form salt and water. it is type of double replacement reaction. (e.g. HCl + NaOH = H2O + NaCl)

60
Q

hydrochloric acid (aqueous hydrogel chloride)

A

HCl(aq)

61
Q

hydrofluoric acid (aqueous hydrogen fluoride)

A

HF(aq)

62
Q

sulphuric acid (aqueous hydrogen sulfate)

A

H2SO4(aq)

63
Q

nitric acid (aqueous hydrogen nitrate)

A

HNO3(aq)

64
Q

carbonic acid (aqueous hydrogen carbonate)

A

H2CO3(aq)

65
Q

acetic acid (aqueous hydrogen acetate, or ethanoic acid)

A

CH3COOH(aq)

66
Q

lye, caustic sode (sodium hydroxide)

A

NaOH(aq)

67
Q

Milk of Magnesia (magnesium hydroxide)

A

Mg(OH)2(aq)

68
Q

lime water (calcium hydroxide)

A

Ca(OH)2(aq)

69
Q

lone pair electrons

A

a pair of valence electrons that are not shared with another atom. Lone pairs are found in the outermost electron shell of atoms. found in Lewis structure.

70
Q

bohr diagram

A

a diagram of an atom which includes all protons, neutrons, electron shells, and electrons

71
Q

lewis diagram

A

a diagram that illustrates chemical bonding by showing only an atom’s valence electrons and its chemical symbol

chemistry grade 10 (1 decks)

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