Chemistry Final Review 10th

stream queencard

1. Chemistry

the study of the composition of matter and the changes that matter undergoes

2. Element

composed of particles called atoms

3. Atom

the basic unit of a chemical element.

4. Compund

A mixture composed of two or more

elements

5. chemical reaction

process in which reactants produce

products

what is produced

6. Mass

A measure of the amount of matter the object contains

7. Mixture

a physical blend of two or more components

8. Mixtures can be classified as

heterogeneous (\`) and homogeneous (\=)

9. homogeneous mixture

a mixture in which the composition is uniform throughout

10. heterogeneous mixture

a mixture in which the composition is NOT uniform throughout

11. Solution

another name for homogeneous mixture

12. chemical symbol

each element is represented by one or two letters

13. Periodic table

an arrangement of elements in which the elements are separated into groups based on a set of repeating properties

14. Period

horizontal row on the periodic table

15. group (family)

Vertical columns on the periodic table

16. Reactant

a substance present at the start of a reaction

17. Product

a substance produced in the reaction

18. precipitate

a solid that forms and settles out of a liquid mixture

19. What does the law of conservation

mass is conserved ; mass is neither tion of matter state? created nor destroyed

20. What is IUPAC?

Organization that sets the standards for chemistry

21. metals

good conductors of heat and electric current

22. non metals

poor conductors of heat and electric current

23. metalloids

Similar to metals and non metals but under some conditions will act like metals and non metals

24. chemical families on periodic

1A-\> Alkali Metals

25. 1A

alkali metals

26. 2A

alkaline earth metals

27. 7A

Halogens

28. 8A

noble gases

29. Noble gases

(Inert gases) rarely takepart in a reaction

30. Transition metals

Group B

31. How do we call the elements in Transition and inner transition metals

group B

32. Inner transition metals

(Appear below the main body) characterized by the presence of electron in f orbital

33. Ion

Atoms with positive or negative charge

34. Cation

positively charged ion

35. Example of Cation

Na^+

36. Anion

negatively charged ion

37. Examples of anion

Cl^-

38. group/familly

vertical (up down)

39. period

horizontal (side to side)

40. Covalent bond

bond formed by the sharing of electrons between atoms

41. Diatomic molecule

a molecule that contains two atoms

42. Seven diatomic elements

hydrogen H2

43. Single Covalent Bond

when two atoms are held together by sharing one pair of electrons

44. Double Covalent Bond

a bond that involves two shared pairs of electrons

45. Triple Covalent Bond

a bond that involves three shared pairs of electrons

46. Polyatomic ion

a tightly bound group of atoms that has a positive or negative charge and behaves as a unit

47. examples of polyatomic ion

(NH4)^+

48. bond dissociation energy

the energy required to break the bond between two covalently bonded atoms

49. molecular orbitals

when 2 atoms combine

50. polar molecule

molecule in width one side of the molecule is slightly negative and the opposite side is slightly positive

51. dipolar molecule/dipole

a molecule that has two sides

52. Van der Waals forces

the two weakest attractions between molecules

53. hydrogen bonds

attractive forces in which a hydrogen covalently bonded to a very electronegative atom

54. ionic compounds

Consist of positively charged ions and negatively charge ions combine in a proportion such that their charges add up to a net charge of zero

55. monoatomic ion

single atoms with a positive or negative charge

56. cations charge

+

57. anions charge

\-

58. method to name ions

stock system

59. Stock system --\>

placing a Roman numeral in parentheses after the name of the element to indicate the value of the charge

60. ex of stock system

Fe^+2 iron (II) ion

61. polyatomic ion

composed of more than one atom

62. how to write the formula of binary

1. write the cation compound 2. write the anion

63. ex of binary compound

K^+ - Cl^\- -\> KCl

64. How to write a compound

1. write the cation polyatomic ion 2. write the anion

65. ex of a compound with a polyatmoic ion

Ca^+2 + (NO3)^\- -\> Ca(NO3)2

66. How do we name and write formulas for molecular compounds ?

1. write the name of 1st element las for molecular compounds ? 2. prefixes to indicate the number of atoms

67. Ex of formulas for molecular com-

CO -\> CO2-\> carbon dioxide S2Cl2 -\>Disulfur dichloride IF7 -\> iodine hepta fluoride

68. How do we name and write acids

- 1. if anion ide -\> hydro+stem anlas ion+ic+acid

69. Ex of formulas for acids

1. HCl hydrochloric acid Sulfurous Acid : 2SO33. Nitric Acid: HNO3

70. How do we name and write formu- 1. Name the cation las for Bases ?

2. follow by the name of the anion

71. Ex of formulas for Bases

NaOH sodium hydroxide Al(OH)3 Aluminium hydroxide

73. guidelines to name a chemical

1. follow the rules for naming acids compound from the chemical for- when its the first element in the formula

74. mole

measurement of matter

75. 1 mol of substance \=

6.02 x 10^23 particle

76. Avogadro's number

6.02 x 10^23

77. representative particle

the species present in a substance

78. molar mass

the atomic mass of an element

79. AMU

atomic mass unit

80. STP

standard temperature and pressure

82. Pressure \=

101.3KPa or 1 atomsphere

83. molecular formula

either the same as the experimental

determined empirical formula

or its a simple whole number multiple

84. Chemical equation

representation of a chemical reaction

85. skeleton equation

a chemical equation that does not indicate the relative amounts of reactants and products

86. first step in writing a chemical

write the skeleton equation equation

87. catalyst

a substance that speeds up the reaction

88. meaning of an arrow

yields / it separates the products from reaction the reactants

89. meaning of a double arrow in a used

place of -\> for reversible reacchemical reaction tions

90. meaning of a triangle

indicate that heat is supplied to the rearrow in a chemical reaction action

91. coefficients

small whole numbers that are placed in front of the formulas in an equation in order to balance it

92. balanced equation

a chemical equation in which mass is conserved

93. combination reaction

2 or more substances react to form a single new substance

94. Ex of combination reaction

Mg+O2-\> 2MgO

95. Decomposition reaction

a single compound breaks down into two or more simpler products

96. ex of decomposition reaction

H2CO3 -\> H2O+CO2

97. single replacement reaction

one element replaces a second element in a compound

98. Ex of single replacement reaction

Zn+Cu(NO3)2 -\> Cu+Zn (NO3)2

99. double replacement reaction

chemical change that involves a change of positive ions between two compounds