Basic concepts in chemistry

some basic concepts related to chemistry.

1. Basic concept of chemistry Kehkashan sabir (lecturer) 1

2. What is chemistry? 2

3. Chemistry is a science that focuses on the composition and properties between a variety of substances and different forms of matter and their interaction with each other. Chemistry is also a physical science that analyzes various atoms, molecules, crystals, and other aggregates of matter. 3

4. biochemistry Biochemistry or biological chemistry, is the study of chemical processes within and relating to living organisms. BIOLOGY CHEMISTRY BIOCHEMISTRY + 4

5. What is nursing ? On the other hand, nursing is an art and science. It interplays with other disciplines outside nursing such as social, behavioral, and physical sciences. Nursing, as a profession is unique because it is focused on health promotion, health maintenance, and health problems of individuals and families. 5

6. Importance of chemistry in nursing 1) Chemistry is important in nursing because it helps in administering medicine to patients. Nurses must understand how particular medicines will react in different patients. This helps to avoid wrong combinations of drugs that can lead to adverse effects. 6

7. 2) Chemistry will also guide the nurse understand the present condition of the patient.  Understanding the importance of Sodium (Na), Potassium (K), Chloride (Cl), Bicarbonate (HCO3), Carbon dioxide (CO2), Oxygen (O), and other electrolytes in the body will guide the nurse to identify if his/her patient is experiencing electrolyte imbalance. 7

8. MORE APPLICATIONS OF CHEMISTRY IN NURSING? 8

9. Basic terms used in chemistry MATTER ATOM ELEMENT MIXTURE COMPOUND 9

10. Matter There are many possible definitions of matter. In science, the matter is the term for any type of material. The matter is anything that has mass and takes up space. At a minimum, the matter requires at least one subatomic particle, although most matter consists of atoms . 10

11. Examples of Matter Matter can include any of the following (and more, of course): Proton Atoms (e.g., a helium atom) Molecules (e.g., water, sugar) Compounds (e.g., table salt, silicon dioxide) Cat Tree House Computer 11

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13. atom How many atoms are there in water? The smallest unit of matter that has the characteristic properties of a chemical element. As such, the atom is the basic building block of chemistry. 13

14. Structure of an Atom Like everything else, atoms have a few different things floating around inside of them. These subatomic particles include: neutrons - with no charge protons - positively charged electrons - negatively charged 14

15. The protons and neutrons are in the atomic nucleus of the atom, while the electrons orbit the atomic nucleus. Think of this as similar to the way the planets all orbit the sun. 15

16. element An atom is the part of an element. A particular element is composed of only one type of atom. Elements can combine with each other to form molecules via chemical reactions. 16

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18. molecules Molecules are what you get when those atoms are combined. Unlike elements, molecules can be made from the same or different elements. The key to a molecule is that two or more atoms are bonded together. 18

19. For example Water is a molecule made of hydrogen and oxygen. It’s actually made of two hydrogen atoms and one oxygen atom. You can also have molecules of a single atom bonded together like two oxygen atoms. This makes up the oxygen humans breathe. 19

20. mixture Mixtures are substances that are formed by physically mixing two or more substances. Mixtures are mainly of two types i.e. homogenous mixtures and heterogeneous mixtures. DIFFERENTIATE BETWEEN HOMOGENOUS AND HETEROGENEOUS MIXTURES WITH EXAMPLES. 20

21. compounds Compounds are substances that can be formed by chemically combining two or more elements. Compounds can be of three types , which are: covalent compounds, metallic compounds, and ionic compounds. Note: Compounds can be classified as organic compounds or inorganic compounds depending on the presence of carbon in the molecular structure. 21

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23. WHAT IS BLOOD ?? IS BLOOD A MIXTURE OR COMPOUND?? 23

24. CHEMICAL FORMULA A chemical formula tells us the number of atoms of each element in a compound. It contains the symbols of the atoms of the elements present in the compound as well as how many there are for each element in the form of subscripts 24

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26. Molecular Formula The molecular formula, sometimes known as the true formula, tells us the actual number of the different elements in one molecule of a compound. In a molecular formula, each element is written as its symbols in the periodic table, and the number of atoms for each element is shown by the subscript (the small number to the lower right of the element). Here are some examples of molecular formulas: 26

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28. EMPIRICAL FORMULA Empirical formula is defined as the simplest ratio of whole numbers of elements that make up a compound, and this type of formula is derived from experimental data. 28

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30. Structural Formula When we simply write the molecular formula, we do not know how the atoms are arranged or which atoms are bonded to each other. The structural formula shows both the actual number of atoms of elements in a compound, how the atoms are arranged and which atoms are bonded to one another. 30

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32. activity Write molecular formula, empirical formula and structural formula of: Water Carbon dioxide Methane Glucose 32

33. Solution Molecular formula Empirical formula Structural formula H 2 H 2 33

34. Molecular Formula Empirical Formula Structural Formula CO 2 CO 2 34

35. Molecular Formula Empirical Formula Structural Formula CH 4 CH 4 35

36. Molecular formula Empirical formula Structural formula C₆H₁₂O₆ CH 2 O 36

37. Chemical reactions A chemical reaction is in which the bonds are broken within reactant molecules, and new bonds are formed within product molecules in order to form a new substance. 37

38. Basic Concepts of Chemical Reactions A Chemical Reaction is a process that occurs when two or more molecules interact to form a new product(s). Compounds that interact to produce new compounds are called reactants whereas the newly formed compounds are called products. Chemical reactions play an integral role in different industries, customs and even in our daily life. They are continuously happening in our general surroundings; for example, rusting of iron, pottery, fermentation of wine and so on. 38

39. In a chemical reaction, a chemical change must occur which is generally observed with physical changes like precipitation, heat production, color change, etc. A reaction can take place between two atoms or ions or molecules, and they form a new bond and no atom is destroyed or created but a new product is formed from reactants. The rate of reaction depends on and is affected by factors like press ure, temperature, the concentration of reactants. 39

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41. 1. Synthesis reactions Two or more reactants combine to make 1 new product. Examples: C(s) + O 2 (g) → CO 2 (g) H 2 O(l) + SO 3 (g) → H 2 SO 4 ( aq ) 41

42. 2. Decomposition reactions A single reactant breaks down to form 2 or more products. Examples: H2CO3 ( aq ) → H2O (l) + CO2 (g) CaCO3 (s) → CaO (s) + CO2 (g) 42

43. 3. Single-replacement reactions A single element replaces a similar element of an adjacent reactant compound. Examples: Zn (s) + CuSO4 ( aq ) → ZnSO4 ( aq ) + Cu (s) 43

44. 4. Double-replacement reactions Two ionic compounds exchange ions, producing 2 new ionic compounds. Examples: NaCl( aq ) AgNO 3 ( aq ) → NaNO 3 ( aq ) + AgCl(s) HCl( aq ) + NaOH( aq ) → NaCl( aq ) + H 2 O(l) 44

45. 5. Combustion reactions A single element or compound combines with oxygen gas releasing energy. This rapid oxidation is called burning. Examples: C (s) + O2 (g) → CO2 (g) + energy 2Mg (s) + O2 (g) → 2MgO (s) + energy 45

46. Chemical equation Chemical equations are symbolic representations of chemical reactions in which the reactants and the products are expressed in terms of their respective chemical formulae. Chemical reactions can be represented on paper with the help of chemical equations, an example for which is represented below (for the reaction between hydrogen gas and oxygen gas to form water). 2H 2 + O 2 → 2H 2 O 46

47. It can also be observed that there are coefficients assigned to each of the symbols of the corresponding reactants and products. 47

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49. Regardless of the absolute numbers of molecules involved, the ratios between the numbers of molecules of each species that react (the reactants) and molecules of each species that form (the products) are the same and are given by the chemical reaction equation. 49

50. Ionic Chemical Equations In ionic chemical equations, the electrolytes (substances that dissociate into ions when dissolved in polar solvents) are split up and written as separate ions. Chemical Equation: CaCl 2 + 2AgNO 3 → Ca(NO3) 2 + 2AgCl↓ Ionic Equation: Ca 2 + + 2Cl– + 2Ag+ + 2NO 3 – → Ca 2 + + 2NO 3 – + 2AgCl↓ 50

51. THANK YOU 51